Chemical Equation Calculations

Size: px
Start display at page:

Download "Chemical Equation Calculations"

Transcription

1 Mole Relationships Chemical Equation Calculations 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol H 2 (g) + Cl 2 (g) 2 HCl(g) 2. Assuming similar conditions, how many liters of chlorine gas react to produce 2 L of hydrogen chloride gas? (a) 1 L (b) 2 L (c) 3 L (d) 4 L H 2 (g) + Cl 2 (g) 2 HCl(g) 3. How many moles of carbon monoxide react with 1 mol of oxygen gas according to the balanced chemical equation? 2 CO(g) + O 2 (g) 2 CO 2 (g) (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol 1

2 4. Assuming similar conditions, how many liters of carbon monoxide gas react to produce 2 L of carbon dioxide gas? 2 CO(g) + O 2 (g) 2 CO 2 (g) (a) 1 L (b) 2 L (c) 3 L (d) 4 L 5. How many moles of water vapor, H 2 O, react with 1 mol of charcoal, C, according to the balanced chemical equation? C(s) + H 2 O(g) CO(g) + H 2 (g) (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol 6. Assuming similar conditions, how many liters of water vapor, H 2 O, react to produce 1 L of hydrogen gas? C(s) + H 2 O(g) CO(g) + H 2 (g) (a) 1 L (b) 2 L (c) 3 L (d) 4 L 7. In an experiment, g of iron metal reacts with g of yellow sulfur. Using the conservation of mass law, predict the mass of product. Fe(s) + S(s) FeS(s) (a) g (b) g (c) g (d) g (e) g 2

3 8. In an experiment, g of charcoal reacts with g of powdered sulfur. Using the conservation of mass law, predict the mass of product. C(s) + 2 S(s) CS 2 (g) (a) g (b) g (c) g (d) g (e) g 9. In an experiment, g of chromium metal reacts with g of iodine. Using the conservation of mass law, predict the mass of product. 2 Cr(s) + 3 I 2 (s) 2 CrI 3 (s) (a) g (b) g (c) g (d) g (e) g 10. In an experiment, g of magnesium reacts to give g magnesium oxide. Using the conservation of mass law, predict the mass of reacting oxygen gas. 2 Mg(s) + O 2 (g) 2 MgO(s) (a) g (b) g (c) g (d) g (e) g 11. In an experiment, g of zinc metal reacts to produce g of zinc oxide. Using the conservation of mass law, predict the mass of reacting oxygen gas. 2 Zn(s) + O 2 (g) 2 ZnO(s) (a) g (b) g (c) g (d) g (e) g 3

4 12. In an experiment, g of gold metal reacts to yield g of gold(iii) chloride. Using the conservation of mass law, predict the mass of reacting chlorine gas. 2 Au(s) + 3 Cl 2 (g) 2 AuCl 3 (s) (a) g (b) g (c) g (d) g (e) g Mole Mole Relationships 13. How many moles of iodine vapor react with 1.00 mol of hydrogen gas? H 2 (g) + I 2 (g) HI(g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 14. How many moles of hydrogen iodide are produced from 1.00 mol of iodine? H 2 (g) + I 2 (g) HI(g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 15. How many moles of hydrogen gas react to yield 1.00 mol of hydrogen iodide? H 2 (g) + I 2 (g) HI(g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 4

5 16. How many moles of water are produced from 1.00 mol of hydrogen peroxide? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 17. How many moles of oxygen are produced from 1.00 mol of hydrogen peroxide? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 18. How many moles of hydrogen peroxide decompose to give 1.00 mol of oxygen? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 19. How many moles of oxygen gas react with 1.00 mol NO? UV NO(g) + O 2 (g) NO 2 (g) (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol 5

6 20. How many moles of nitrogen dioxide gas are produced from 1.00 mol NO? UV NO(g) + O 2 (g) NO 2 (g) (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol 21. How many moles of oxygen gas react to yield 1.00 mol NO 2? UV NO(g) + O 2 (g) NO 2 (g) (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol 22. How many moles of water react with 5.00 mol of lithium metal? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g) 23. How many moles of hydrogen gas are produced from 5.00 mol of water? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g) 6

7 24. How many moles of lithium metal react to yield 5.00 mol of hydrogen gas? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g) 25. How many moles of water react with mol of calcium metal? (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g) 26. How many moles of hydrogen gas are produced from mol of water? (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g) 27. How many moles of calcium metal react to yield mol of hydrogen gas? (a) mol (b) mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g) 7

8 28. How many moles of oxygen gas react with mol of pentane, C 5 H 12? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) mol (b) mol (c) mol (d) mol 29. How many moles of water are produced from mol pentane, C 5 H 12? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) mol (b) mol (c) mol (d) mol 30. How many moles of oxygen gas react to yield mol water? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) mol (b) mol (c) mol (d) mol Types of Stoichiometry Problems Mass Mass Problems 47. What is the mass of silver metal produced from 6.35 g of copper? (a) g (b) g (c) g (d) 1.08 g (e) 21.6 g Cu(s) + AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + Ag(s) 8

9 48. What is the mass of copper metal that yields g of silver? (a) g (b) g (c) g (d) g (e) 1.70 g Cu(s) + AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + Ag(s) 49. What is the mass of silver bromide ( g/mol) precipitated from 2.96 g of iron(iii) bromide ( g/mol)? (a) g (b) g (c) 1.88 g (d) 5.64 g (e) 3.76 g FeBr 3 (s) + AgNO 3 (aq) AgBr(s) + Fe(NO 3 ) 3 (aq) 50. What is the mass of iron(iii) bromide ( g/mol) that yields g of silver bromide ( g/mol) precipitate? (a) g (b) g (c) g (d) g (e) g FeBr 3 (s) + AgNO 3 (aq) AgBr(s) + Fe(NO 3 ) 3 (aq) 51. What is the mass of lead(ii) iodide (461.0 g/mol) precipitated from g of potassium iodide ( g/mol)? (a) g (b) g (c) 1.15 g (d) 2.31 g (e) 4.61 g Pb(NO 3 ) 2 (aq) + KI(s) PbI 2 (s) + KNO 3 (aq) 9

10 52. What is the mass of potassium iodide ( g/mol) that yields g of lead(ii) iodide (461.0 g/mol) precipitate? (a) g (b) g (c) g (d) g (e) 2.78 g Pb(NO 3 ) 2 (aq) + KI(s) PbI 2 (s) + KNO 3 (aq) 53. What is the mass of insoluble calcium phosphate ( g/mol) produced from g of calcium chloride ( g/mol)? (a) g (b) g (c) g (d) 1.55 g (e) 4.65 g CaCl 2 (s) + Na 3 PO 4 (aq) Ca 3 (PO 4 ) 2 (s) + NaCl(aq) 54. What is the mass of sodium phosphate ( g/mol) that yields 1.00 g of calcium phosphate ( g/mol) precipitate? (a) g (b) g (c) g (d) 1.06 g (e) 8.38 g CaCl 2 (s) + Na 3 PO 4 (aq) Ca 3 (PO 4 ) 2 (s) + NaCl(aq) 55. What is the mass of aluminum oxide ( g/mol) produced from 3.59 g of iron(ii) oxide (71.85 g/mol)? FeO(l) + Al(l) Fe(l) + Al 2 O 3 (l) (a) g (b) 1.70 g (c) 5.10 g (d) 7.58 g (e) 15.3 g 10

11 56. What is the mass of aluminum metal that reacts to give 1.00 g of iron? FeO(l) + Al(l) Fe(l) + Al 2 O 3 (l) (a) g (b) g (c) g (d) g (e) g 57. What is the mass of aluminum oxide ( g/mol) produced from 1.74 g of manganese(iv) oxide (86.94 g/mol)? MnO 2 (l) + Al(l) Mn(l) + Al 2 O 3 (l) (a) g (b) 1.36 g (c) 2.04 g (d) 2.22 g (e) 3.06 g 58. What is the mass of aluminum metal that reacts to give 11.1 g of manganese metal? MnO 2 (l) + Al(l) Mn(l) + Al 2 O 3 (l) (a) 3.64 g (b) 4.09 g (c) 5.45 g (d) 7.27 g (e) 8.18 g 59. What is the mass of hydrogen gas released from 2.70 g of aluminum metal and hydrochloric acid? (a) g (b) g (c) g (d) g (e) g Al(s) + HCl(aq) AlCl 3 (aq) + H 2 (g) 11

12 60. What is the mass of aluminum metal that reacts to give 1.00 g of hydrogen gas? (a) 4.46 g (b) 8.90 g (c) 13.4 g (d) 20.0 g (e) 26.7 g Al(s) + HCl(aq) AlCl 3 (aq) + H 2 (g) The Limiting Reactant Concept 85. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 1.00 mol A and 1.00 mol B? (a) 1.00 mol (b) 1.50 mol (c) 2.00 mol (d) 3.00 mol A(g) + 2 B(g) 3 C(g) 86. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 1.50 mol A and 3.50 mol B? (a) 1.50 mol (b) 3.50 mol (c) 4.50 mol (d) 5.25 mol A(g) + 2 B(g) 3 C(g) 87. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 2.00 mol A and 4.50 mol B? (a) 2.00 mol (b) 3.00 mol (c) 4.00 mol (d) 4.50 mol A(g) + 3 B(g) 2 C(g) 12

13 88. Considering the limiting reactant concept, how many moles of copper(i) sulfide are produced from the reaction of 1.00 mol of copper and 1.00 mol of sulfur? 2 Cu(s) + S(s) Cu 2 S(s) (a) mol (b) 1.00 mol (c) 1.50 mol (d) 2.00 mol 89. Considering the limiting reactant concept, how many moles of copper(i) sulfide are produced from the reaction of 3.00 mol of copper and 1.00 mol of sulfur? 2 Cu(s) + S(s) Cu 2 S(s) (a) 1.00 mol (b) 1.50 mol (c) 4.00 mol (d) 6.00 mol 90. Considering the limiting reactant concept, how many moles of cobalt(iii) oxide are produced from the reaction of 1.00 mol of cobalt and 1.00 mol of oxygen gas? 4 Co(s) + 3 O 2 (g) 2 Co 2 O 3 (s) (a) mol (b) mol (c) 1.50 mol (d) 2.00 mol Limiting Reactant Problems 91. Considering the limiting reactant, what is the mass of zinc sulfide (97.46 g/mol) produced from g of zinc and g of sulfur? Zn(s) + S(s) ZnS(s) (a) g (b) 1.12 g (c) 1.50 g (d) 2.24 g (e) 2.28 g 13

14 92. Considering the limiting reactant, what is the mass of zinc sulfide (97.46 g/mol) produced from g of zinc and g of sulfur? Zn(s) + S(s) ZnS(s) (a) g (b) 1.06 g (c) 1.10 g (d) 1.12 g (e) 2.28 g 93. Considering the limiting reactant, what mass of cobalt(iii) sulfide ( g/mol) is produced from g of cobalt and g of sulfur? 2 Co(s) + 3 S(s) Co 2 S 3 (s) (a) g (b) 1.36 g (c) 2.34 g (d) 2.72 g (e) 5.45 g 94. Considering the limiting reactant, what is the mass of iron produced from 75.0 g of ferrous oxide (71.85 g/mol) and 25.0 g of magnesium metal? FeO(s) + Mg(s) Fe(l) + MgO(s) (a) 28.7 g (b) 29.1 g (c) 57.4 g (d) 58.3 g (e) g 95. Considering the limiting reactant, what is the mass of iron produced from 80.0 g of ferrous oxide (71.85 g/mol) and 20.0 g of magnesium metal? FeO(s) + Mg(s) Fe(l) + MgO(s) (a) 23.0 g (b) 31.1 g (c) 45.9 g (d) 62.2 g (e) g 14

15 96. Considering the limiting reactant, what is the mass of manganese produced from 25.0 g of manganese(iv) oxide (86.94 g/mol) and 25.0 g of aluminum metal? 3 MnO 2 (s) + 4 Al(s) 3 Mn(l) + 2 Al 2 O 3 (s) (a) 15.8 g (b) 38.2 g (c) 47.4 g (d) 50.9 g (e) 67.8 g Note: When working with gases you can use volumes instead of moles. 97. Considering the limiting reactant, what is the volume of NO gas produced from 30.0 L of nitrogen gas and 40.0 L of oxygen gas? (Assume constant conditions.) N 2 (g) + O 2 (g) 2 NO(g) (a) 30.0 L (b) 40.0 L (c) 60.0 L (d) 80.0 L 98. Considering the limiting reactant, what is the volume of NO gas produced from 30.0 L of nitrogen gas and 20.0 L of oxygen gas? (Assume constant conditions.) N 2 (g) + O 2 (g) 2 NO(g) (a) 20.0 L (b) 30.0 L (c) 40.0 L (d) 60.0 L 99. Considering the limiting reactant, what is the volume of NO 2 gas produced from 3.00 L of NO gas and 2.00 L of oxygen gas? (Assume constant conditions.) 2 NO(g) + O 2 (g) 2 NO 2 (g) (a) 1.00 L (b) 2.00 L (c) 3.00 L (d) 4.00 L 15

16 100. Considering the limiting reactant, what is the volume of NO gas produced from 40.0 L of ammonia gas and 40.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 32.0 L (b) 40.0 L (c) 50.0 L (d) 80.0 L 101. Considering the limiting reactant, what is the volume of NO gas produced from 50.0 L of ammonia gas and 60.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 48.0 L (b) 50.0 L (c) 60.0 L (d) 75.0 L 102. Considering the limiting reactant, what is the volume of NO gas produced from 60.0 L of ammonia gas and 50.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 40.0 L (b) 50.0 L (c) 60.0 L (d) 62.5 L Empirical Formula 85. If mol of copper combines with mol of sulfur, what is the empirical formula of the copper sulfide product? (a) CuS (b) Cu 2 S (c) CuS 2 (d) Cu 5 S 5 16

17 86. If mol of lead combines with mol of sulfur, what is the empirical formula of the lead sulfide product? (a) PbS (b) Pb 2 S (c) PbS 2 (d) Pb 3 S If mol of tin combines with mol of sulfur, what is the empirical formula of the tin sulfide product? (a) SnS (b) Sn 2 S (c) SnS 2 (d) Sn 3 S If 6.00 mol of cobalt combines with 9.00 mol of sulfur, what is the empirical formula of the cobalt sulfide product? (a) Co 2 S 3 (b) Co 3 S 2 (c) Co 6 S 9 (d) Co 9 S If mol of red phosphorus reacts with mol of yellow sulfur, what is the empirical formula of the product? (a) P 2 S 3 (b) P 2 S 5 (c) P 3 S 2 (d) P 5 S If mol of red phosphorus reacts with mol of yellow sulfur, what is the empirical formula of the product? (a) P 2 S 3 (b) P 2 S 5 (c) P 3 S 2 (d) P 5 S 2 17

18 91. If g of nickel metal reacts with g of chlorine gas, what is the empirical formula of the nickel chloride product? (a) NiCl (b) NiCl 2 (c) NiCl 3 (d) Ni 2 Cl 3 (e) Ni 3 Cl If g of cobalt metal react with g of oxygen gas, what is the empirical formula of the cobalt oxide product? (a) CoO (b) CoO 2 (c) CoO 3 (d) Co 2 O 3 (e) Co 3 O If g of cobalt metal react with g of oxygen gas, what is the empirical formula of the cobalt oxide product? (a) CoO (b) CoO 2 (c) CoO 3 (d) Co 2 O 3 (e) Co 3 O If g of tin metal reacts with g of fluorine gas, what is the empirical formula of the product? (a) SnF (b) SnF 2 (c) SnF 4 (d) SnF 10 (e) Sn 2 F If g of bismuth metal react with sulfur to give g of bismuth sulfide, what is the empirical formula of the product? (a) BiS (b) BiS 2 (c) BiS 3 (d) Bi 2 S 3 (e) Bi 3 S 2 18

19 96. If g of vanadium metal react with oxygen gas to give g of vanadium oxide, what is the empirical formula of the product? (a) VO (b) V 2 O 3 (c) V 2 O 5 (d) V 3 O 2 (e) V 5 O Acetylene is used in oxyacetylene gas welding. Calculate the empirical formula for acetylene given its percent composition: 92.25% C and 7.75% H. (a) CH (b) CH 2 (c) CH 8 (d) C 8 H 8 (e) C 12 H 98. Fructose is a sugar found in fruit and honey. Calculate the empirical formula for fructose given its percent composition: 40.00% C, 6.72% H, and 53.29% O. (a) CHO (b) CH 2 O (c) CHO 2 (d) C 3 H 6 O 3 (e) C 6 HO Butyric acid is the odor of rancid cheese. Calculate the empirical formula for butyric acid given its percent composition: 54.53% C, 9.15% H, and 36.32% O. (a) CHO (b) C 2 H 4 O (c) C 2 H 3 O (d) C 5 H 9 O 2 (e) C 6 H 9 O 3 19

20 Mole Relationships 1. A 2. A 3. B 4. B 5. A 6. A 7. D 8. C 9. C 10. B 11. B 12. B Mol-Mol Relationship 13. B 14. C 15. A 16. B 17. A 18. C 19. B 20. C 21. B 22. B 23. A 24. C 25. C 26. A 27. B 28. D 29. C 30. E Mass-Mass Problems 47. E 48. A 49. D 50. A 51. C 52. C 53. B 54. D 55. B 56. A 57. B 58. D 59. D 60. B 61. A 62. E 63. A 64. E 65. D 66. B 67. A 68. E 69. E 70. C 71. D 72. B 73. C 74. E Lim. React. Concept 85. B 86. C 87. B 88. A 89. A 90. A Lim. React Problems 91. B 92. B 93. A 94. C 95. C 96. A 97. C 98. C 99. C 100. A 101. A 102. A Empirical Formulas 85. B 86. A 87. C 88. A 89. A 90. B 91. C 92. A 93. D 94. C 95. D 96. C 97. A 98. B 99. B 20

Moles, Mass, and Limiting Reactants

Moles, Mass, and Limiting Reactants Moles, Mass, and Limiting Reactants Interpreting a Chemical Equation 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol

More information

Moles, Mass, and Limiting Reactants

Moles, Mass, and Limiting Reactants Moles, Mass, and Limiting Reactants Answers follow at end Interpreting a Chemical Equation) 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according tothe balanced chemical equation?

More information

Study Guide: Stoichiometry

Study Guide: Stoichiometry Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE

More information

Reaction Writing Sheet #1 Key

Reaction Writing Sheet #1 Key Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium

More information

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date» Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent

More information

IB Topics 9 & 19 Multiple Choice Practice

IB Topics 9 & 19 Multiple Choice Practice IB Topics 9 & 19 Multiple Choice Practice 1. What are the oxidation states of chromium in (NH 4) 2Cr 2O 7 (s) and Cr 2O 3 (s)? 2. Which of the following is a redox reaction? 3Mg (s) + 2AlCl 3 (aq) 2Al

More information

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question.

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question. Unit 4 Multiple Choice Identify the choice that best completes the statement or answers the question. 39. Changing a subscript in a correctly written chemical formula a. changes the number of moles represented

More information

Unit 4: Reactions and Stoichiometry

Unit 4: Reactions and Stoichiometry Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)

More information

Stoichiometric Calculations

Stoichiometric Calculations Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Slide 4 / 109 Table of Contents Stoichiometry Calculations with Moles Click on the topic to go to that section Stoichiometry Calculations

More information

Stoichiometric Calculations

Stoichiometric Calculations Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Table of Contents Click on the topic to go to that section Stoichiometry Calculations with Moles Stoichiometry Calculations with Particles

More information

UNIT 9 - STOICHIOMETRY

UNIT 9 - STOICHIOMETRY General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information

UNIT 1 Chemical Reactions Part II Workbook. Name:

UNIT 1 Chemical Reactions Part II Workbook. Name: UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the

More information

Exe r c i s es Answers to odd-numbered Exercises are in Appendix I. Key Te rm s Answers to Key Terms are in Appendix H.

Exe r c i s es Answers to odd-numbered Exercises are in Appendix I. Key Te rm s Answers to Key Terms are in Appendix H. 284 CHAPTER 10 CHEMICAL EQUATION CALCULATIONS Moles reactant (b) 'llljll!llim'.lllill!w 11r1 nrr1111 Moles product.,.. Concept Map-Summary Stoichiometry We use a strategy map to show the application unit

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

11.2 Types of Chemical Reactions> Chapter 11 Chemical Reactions Types of Chemical Reactions Describing Chemical Reactions

11.2 Types of Chemical Reactions> Chapter 11 Chemical Reactions Types of Chemical Reactions Describing Chemical Reactions Chapter 11 Chemical 11.1 Describing Chemical 11.2 Types of Chemical 11.3 in Aqueous Solution 1 CHEMISTRY & YOU What happens to the wax when you burn a candle? When you burn a candle, a chemical reaction

More information

Chapter 8 Chemical Reactions

Chapter 8 Chemical Reactions Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3? 1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K

More information

Ch. 8 Chemical Reactions

Ch. 8 Chemical Reactions Ch. 8 Chemical Reactions Intro to Reactions I II III IV V Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change Law of Conservation of Mass

More information

Chapter 7: Stoichiometry in Chemical Reactions

Chapter 7: Stoichiometry in Chemical Reactions Chapter 7: Stoichiometry in Chemical Reactions Mini Investigation: Precipitating Ratios, page 315 A. ZnCl 2 (aq) + Na 2 CO 3 (aq) ZnCO 3 (s) + 2 NaCl(aq) 3 AgNO 3 (aq) + Na 3 PO 4 (aq) Ag 3 PO 4 (s) +

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

CHAPTER 11 Stoichiometry Defining Stoichiometry

CHAPTER 11 Stoichiometry Defining Stoichiometry CHAPTER 11 Stoichiometry 11.1 Defining Stoichiometry Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry

More information

Example Exercise 10.1 Interpreting Chemical Equation Calculations

Example Exercise 10.1 Interpreting Chemical Equation Calculations Example Exercise 10.1 Interpreting Chemical Equation Calculations Given the chemical equation for the combustion of methane, CH 4, balance the equation and interpret the coefficients in terms of (a) moles

More information

2H 2 (g) + O 2 (g) 2H 2 O (g)

2H 2 (g) + O 2 (g) 2H 2 O (g) Mass A AP Chemistry Stoichiometry Review Pages Mass to Mass Stoichiometry Problem (Review) Moles A Moles B Mass B Mass of given Amount of given Amount of unknown Mass of unknown in grams in Moles in moles

More information

Unit 9 Stoichiometry Notes

Unit 9 Stoichiometry Notes Unit 9 Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations to

More information

SCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4

SCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4 Lesson Topics Covered 1 Note: Chemical Reactions and Chemical Equations definition of chemical reaction four signs of chemical change the Law of Conservation of Mass balancing chemical equations SCH 3UI

More information

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Formulas and Chemical Nomenclature Mr. Matthew Totaro Legacy High School Honors Chemistry 1 Molecular View of Elements and Compounds 2 Atomic Elements Atomic Elements = elements whose smallest

More information

Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions

Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In

More information

Electrodeposition. - Worksheet - Envisioning Chemistry. 1. Write half reactions for the following processes under electrical current.

Electrodeposition. - Worksheet - Envisioning Chemistry. 1. Write half reactions for the following processes under electrical current. Electrodeposition 1. Write half reactions for the following processes under electrical current. (1). Formation of copper from copper (II) ion Example: Cu 2+ + 2e --> Cu (2). Formation of tin from tin ion

More information

Calculating equilibrium constants

Calculating equilibrium constants Equilibrium Work Book Writing Equilibrium Constants Expressions 1. Write the equilibrium law (mass action expression) for each of the following reactions: a. SO 2 (g) + NO 2 (g) SO 3 (g) + NO(g) b. 2 C(s)

More information

Unit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations

Unit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations Unit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations 1. Describe the following word equation with a statement or sentence: Iron + Oxygen iron (III) oxide 2. In a

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:

More information

Reactions in aqueous solutions Redox reactions

Reactions in aqueous solutions Redox reactions Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and

More information

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide. Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the

More information

c formula units of potassium iodide a moles of beryllium b moles of calcium c mole of sulfur a. 6.

c formula units of potassium iodide a moles of beryllium b moles of calcium c mole of sulfur a. 6. Chapter 11 1. Identify and calculate the number of representative particles in each of the following quantities. a. 2.15 moles of gold 2.15 mol Au 1.29 10 24 atoms Au b. 0.151 mole of nitrogen oxide 0.15O

More information

SCH4U Chemistry Review: Fundamentals

SCH4U Chemistry Review: Fundamentals SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.

More information

Chemical Reactions CHAPTER Reactions and Equations

Chemical Reactions CHAPTER Reactions and Equations CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number

More information

Danyal Education (Contact: ) A commitment to teach and nurture

Danyal Education (Contact: ) A commitment to teach and nurture Chemistry of Reactions: Redox (#) Candidates should be able to: a) define oxidation and reduction (redox) in terms of oxygen/hydrogen gain/loss b) define redox in terms of electron transfer and changes

More information

Name Period CH 180 Practice Test: Chapters 3 and 4

Name Period CH 180 Practice Test: Chapters 3 and 4 Name Period CH 180 Practice Test: Chapters 3 and 4 Multiple Choice: 1. 11. 2. 12. 3. 13. 4. 14. 5. 15. 6. 16. 7. 17. 8. 18. 9. 19. 10. 20. 21. 22. 23. 24. 25. 26. 27. 1 Directions: Answer all questions.

More information

(DO NOT WRITE ON THIS TEST)

(DO NOT WRITE ON THIS TEST) Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation

More information

Unit Two Worksheet WS DC U2

Unit Two Worksheet WS DC U2 Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed

More information

Unit 8 Chemical Reactions- Funsheets

Unit 8 Chemical Reactions- Funsheets Part A- Balancing Equations and Types of Reactions Balance AND identify the following reactions: Unit 8 Chemical Reactions- Funsheets 1) Mg + Zn(NO 3) 2 Zn Mg(NO 3) 2 2) Ba + AgNO 3 Ag + Ba(NO 3) 2 3)

More information

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES 5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write

More information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information 12 Study Guide 12 Study Guide Study Tip Prioritize Schedule your time realistically. Stick to your deadlines. If your class subscribes to the Interactive Textbook with ChemASAP, your students can go online

More information

Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change.

Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. Chemical Reactions I. What is a chemical reaction? Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. A. How can you

More information

Chem!stry. Assignment on Redox

Chem!stry. Assignment on Redox Chem!stry Name: ( ) Class: Date: / / Assignment on Redox Question 1: Which one of the following elements is the most powerful reducing agent? A Aluminium B Copper C Lead D Potassium Question 2: Which of

More information

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 )

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 ) Homework Stoichiometry 1.) An oxide of iron has the formula Fe 3 O 4. What mass percent of iron does it contain? (72.360%) 2.) Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed

More information

Balancing CHEMICAL EQUATIONS

Balancing CHEMICAL EQUATIONS Balancing CHEMICAL EQUATIONS CHEMICAL REACTIONS involves a chemical change in the identity of one or more chemical species Ex. Rusting of iron (Fe): chemical rxn btwn water and iron involve the breaking

More information

Name AP Chemistry September 30, 2013

Name AP Chemistry September 30, 2013 Name AP Chemistry September 30, 2013 AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the blue side of your scantron for each of the

More information

2. Indicators of Chemical Rxns. Abbreviations of State (g) gas (l) liquid (s) solid (aq) aqueous a substance dissolved in water

2. Indicators of Chemical Rxns. Abbreviations of State (g) gas (l) liquid (s) solid (aq) aqueous a substance dissolved in water Unit 6 Chemical Reactions 1. Parts of a Chemical Reaction 2. Indicators of a Chemical Reaction 3. Enthalpy 4. Balancing Chemical Equations 5. Word Equations 6. Classifying Chemical Reactions 7. Predicting

More information

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +

More information

1. Parts of Chemical Reactions. 2 H 2 (g) + O 2 (g) 2 H 2 O(g) How to read a chemical equation

1. Parts of Chemical Reactions. 2 H 2 (g) + O 2 (g) 2 H 2 O(g) How to read a chemical equation Unit 6 Chemical Reactions 1. Parts of a Chemical Reaction 2. Indicators of a Chemical Reaction 3. Enthalpy 4. Balancing Chemical Equations 5. Word Equations 6. Classifying Chemical Reactions 7. Predicting

More information

TYPES OF CHEMICAL REACTIONS

TYPES OF CHEMICAL REACTIONS TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility

More information

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of

More information

Topic 8: Chemical Reactions Chemical Equations & Reactions

Topic 8: Chemical Reactions Chemical Equations & Reactions Topic 8: Chemical Reactions Chemical Equations & Reactions (Chapter 8 in Modern Chemistry) Describing Chemical Reactions A chemical reaction is the process by which one or more substances are changed into

More information

5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams.

5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams. CHEMISTRY TEST NAME: MASS AND VOLUME DATE: EQUATION RELATIONSHIPS Directions: For each of the following questions, choose the number that best answers the question and place it on your answer sheet. Directions:

More information

Exam III Material Chapter 7-CHEMICAL REACTIONS, continued

Exam III Material Chapter 7-CHEMICAL REACTIONS, continued Exam III Material Chapter 7-CHEMICAL REACTIONS, continued A chemical reaction occurs when there is a change in chemical composition. I. Double Replacement/Double Exchange/Metathesis Reactions In an double

More information

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters] 1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

EXAM 3 CHEM 1310 WS09 Key Version #2

EXAM 3 CHEM 1310 WS09 Key Version #2 EXAM 3 CHEM 1310 WS09 Key Version #2 1. (p. 116) Select the correct name and chemical formula for the precipitate that forms when the following reactants are mixed. CuCl 2 (aq) + Na 2 CO 3 (aq) A. copper(ii)

More information

Gravimetric Analysis (Analysis by Mass)

Gravimetric Analysis (Analysis by Mass) Week 2 Measuring water content Gravimetric Analysis (Analysis by Mass Water is a component in many consumer products It may occur naturally or may be added in manufacturing Water content can reveal the

More information

Unit 10: Stoichiometry Funsheets. Part A: Balanced Chemical Equations- Balance the following chemical equations.

Unit 10: Stoichiometry Funsheets. Part A: Balanced Chemical Equations- Balance the following chemical equations. Unit 10: Stoichiometry Funsheets Part A: Balanced Chemical Equations- Balance the following chemical equations. 1) Al + Cl 2 AlCl 3 2) Mg(ClO) 2 MgCl 2 + O 2 3) FeCl 3 + LiOH Fe(OH) 3 + LiCl 4) Na + O

More information

CHM 134 General Chemistry I Exam 2 Review, Dr. Steel. 1. Give the oxidation number of sulfur in each of these compounds.

CHM 134 General Chemistry I Exam 2 Review, Dr. Steel. 1. Give the oxidation number of sulfur in each of these compounds. CHM 1 General Chemistry I Exam Review, Dr. Steel Name 1. Give the oxidation number of sulfur in each of these compounds. H S SO H SO SO -. In the lab you reacted magnesium metal and oxygen gas to produce

More information

Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds.

Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using

More information

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic

More information

BALANCING EQUATIONS NOTES

BALANCING EQUATIONS NOTES BALANCING EQUATIONS NOTES WHY DO WE NEED TO BALANCE CHEMICAL EQUATIONS? The LAW OF CONSERVATION OF MASS says that matter cannot be created or destroyed. In other words, you cannot end up with any more

More information

Name Date Class THE ARITHMETIC OF EQUATIONS

Name Date Class THE ARITHMETIC OF EQUATIONS 12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in terms of interacting

More information

CHAPTER 9 CHEMICAL QUANTITIES

CHAPTER 9 CHEMICAL QUANTITIES Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Chemistry 2202 Stoichiometry Unit Retest Review Guide

Chemistry 2202 Stoichiometry Unit Retest Review Guide Chemistry 2202 Stoichiometry Unit Retest Review Guide Chapter 2: The Mole Pgs. 42 77 You should be able to: 1. Define the term molar mass and calculate the molar mass of any given element or compound.

More information

elemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.

elemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another. CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two

More information

Chapter 9 - Reactions

Chapter 9 - Reactions Chapter 9 - Reactions How many different elements are in: MgBr 2 NH 4 OH CH 3 OH CH 3 CH 2 OH CH 3 COOH Sr(NO 3 ) 2 How many atoms are represented by: K 2 S Li 3 PO 4 Sr(OH) 2 Fe(NO 3 ) 3 Al 2 (SO 4 )

More information

STOICHIOMETRY CLASSWORK

STOICHIOMETRY CLASSWORK STOICHIOMETRY CLASSWORK Given the following equation: 2 C4H10 + 13 02 ---> 8 CO2 + 10 H20 Show what the following molar ratios should be. a, C4H10 / 02 b. 02 / CO2 o, 02 / H20 d, C4Hlo / CO2 e. C4Hlo /

More information

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the

More information

CHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion.

CHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. CHAPTER 8 SALTS A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. The salt consists of two parts, cation from base and anion from acid.

More information

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4 Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react

More information

Practice Problems: Set #3-Solutions

Practice Problems: Set #3-Solutions Practice Problems: Set #3-Solutions IIa) Balance the following equations:(10) 1) Zn (s) + H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + H 2 (g) 3Zn (s) + 2H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + 3H 2 (g) 2. Mg 3 N 2 (s)

More information

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D % 1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16

More information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri

Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How

More information

Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations

Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations Stoichiometry Table of Contents Section 1 Introduction to Stoichiometry Section 2 Ideal Stoichiometric Calculations Section 3 Limiting Reactants and Percentage Yield Section 1 Introduction to Stoichiometry

More information

Nomenclature Naming Ionic Compounds Worksheet #1

Nomenclature Naming Ionic Compounds Worksheet #1 Naming Ionic Compounds Worksheet #1 In forming ionic compounds with non-metals, the transition metals often exhibit more than one valence. For example, in the reaction between iron and chlorine, two products

More information

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022 CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)

More information

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O

More information

Unit IV: Chemical Equations & Stoichiometry

Unit IV: Chemical Equations & Stoichiometry Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations

More information

UNIT 9 - STOICHIOMETRY

UNIT 9 - STOICHIOMETRY General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. Atomic mass

More information

Closed Book Exam - No books or notes allowed. All work must be shown for full credit. You may use a calculator.

Closed Book Exam - No books or notes allowed. All work must be shown for full credit. You may use a calculator. Chem 110 Name Exam #4 April 1, 2017 Closed Book Exam - No books or notes allowed. All work must be shown for full credit. You may use a calculator. Question Part I (40) Part II (60) Credit TOTAL Part I

More information

9-1 The Nature of Chemical Reactions

9-1 The Nature of Chemical Reactions 9-1 The Nature of Chemical Reactions What are chemical reactions and why do they occur? A chemical reaction is a process in which one or more substances are converted into new substances with different

More information

THE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

THE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. THE MOLE - PART 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which one of the following statements is a quantitative observation? a.

More information

Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products)

Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products) Unit 8: Balancing and Identifying Chemical Reactions Packet Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products) C O 2 CO

More information

Exam 1 Worksheet Chemistry 102

Exam 1 Worksheet Chemistry 102 Exam 1 Worksheet Chemistry 102 Chapter 1 Introduction 1. Convert: a. 650 nm to inches b. 650 km to miles c. 345 mg to lb d. 145 lb to μg e. 4.50 10 10 km to μm f. 8.09 10 8 mg to Mg g. 9.00 10 5 ml to

More information

CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.

CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best

More information

Chemical Equations and Chemical Reactions

Chemical Equations and Chemical Reactions Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of

More information

Chemical Reactions. Chemical changes are occurring around us all the time

Chemical Reactions. Chemical changes are occurring around us all the time Chemical changes are occurring around us all the time Food cooking Fuel being burned in a car s engine Oxygen being used in the human body The starting materials are called reactants The ending materials

More information

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Proportions in Chemical Compounds

Proportions in Chemical Compounds Chapter 6 Proportions in Chemical Compounds Section 6.1 Chemical Proportions and Percentage Composition Solutions for Practice Problems Student Edition page 260 1. Practice Problem (page 260) Calculate

More information

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most

More information

REVIEW OF BASIC CHEMISTRY ANSWER KEY

REVIEW OF BASIC CHEMISTRY ANSWER KEY REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F

More information

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the

More information