Study Guide: Stoichiometry

Transcription

1 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 IN QUESTIONS 5 14: 1. Al + O 2 Al 2 O 3 2. Cu + AgNO 3 Ag + Cu(NO 3 ) 2 3. Zn + HCl ZnCl 2 + H 2 4. Fe + Cl 2 FeCl 3 PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS: 5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How many moles of HCl are required to produce 7.50 moles of ZnCl 2? 6. Copper metal reacts with silver nitrate to form silver and copper(ii) nitrate. How many grams of copper are required to form 250 g of silver? 7. When aluminum is burned in excess oxygen, aluminum oxide is produced. How many grams of oxygen are required to produce 0.75 moles of Al 2 O 3? 8. How many grams of iron(iii) chloride are produced when 15.3 g of iron react with excess chlorine gas? 9. When 9.34 g of zinc react with excess hydrochloric acid how many grams of zinc chloride will be produced?

2 PERFORM THE FOLLOWING LIMITING REACTANT PROBLEMS: 10. When 16.3 g of magnesium and 4.52 g of oxygen gas react, how many grams of magnesium oxide will be formed? Identify the limiting and excess reactants. 2 Mg + O 2 2 MgO 11. If 25.3 g of aluminum reacts with 25.3 g of copper(ii) sulfate, how many grams of copper are formed? Identify the limiting and excess reactants in this single replacement reaction. 2 Al + 3 CuSO 4 3 Cu + Al 2 (SO 4 ) Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 ml of 0.250M Pb(NO 3 ) 2. How many grams of lead are formed in this single replacement reaction? Zn + Pb(NO 3 ) 2 Pb + Zn(NO 3 ) If 24.5 g of iron are placed in 1.00 L of 0.25M HCl, how many grams of FeCl 2 are obtained? Identify the limiting and excess reactants in this single replacement reaction. Fe + 2 HCl FeCl 2 + H 2 PERFORM THE FOLLOWING PERCENT YIELD CALCULATIONS: 14. If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of oxygen gas are also given off. Find the theoretical and percent yields. 2 KClO 3 2 KCl + 3 O 2

3 Stoichiometry Review Ch. 9 ANSWER KEY BALANCED EQUATIONS 1. 4 Al + 3 O 2 2 Al 2 O 3 2. Cu + 2 AgNO 3 2 Ag + Cu(NO 3 ) 2 3. Zn + 2 HCl ZnCl 2 + H Fe + 3 Cl 2 2 FeCl 3 STOICHIOMETRIC CALCULATIONS mol HCl g Cu g O g FeCl g ZnCl 2 LIMITING REACTANT 10. LR: O 2 XS: Mg Product: 11.4 g MgO 11. LR: CuSO 4 XS: Al Product: 10.0 g Cu 12. LR: Zn XS: Pb(NO 3 ) 2 Product: 3.17 g Pb 13. LR: HCl XS: Fe Product: 16 g FeCl 2 PERCENT YIELD 14. Theoretical: 2.13 g O 2 Percent Yield: 82.2%

4 Chemical Reactions Review IDENTIFY THE TYPE OF REACTION AND BALANCE THE EQUATION: 1. Sb + I 2 SbI 3 2. Li + H 2 O LiOH + H 2 3. AlCl 3 Al + Cl 2 5. AlCl 3 + Na 2 CO 3 Al 2 (CO 3 ) 3 + NaCl 6. HNO 3 + Ba(OH) 2 Ba(NO 3 ) 2 + H 2 O 7. Al + Pb(NO 3 ) 2 Al(NO 3 ) 3 + Pb 4. C 6 H 12 + O 2 CO 2 + H 2 O IDENTIFY THE TYPE OF REACTION & WRITE A BALANCED EQUATION (INCL. STATES): 8. Aqueous solutions of ammonium chloride and lead(ii) nitrate produce lead(ii) chloride precipitate and aqueous ammonium nitrate. 9. Solid carbon disulfide burns in oxygen to yield carbon dioxide and sulfur dioxide gases. 10. Iron metal reacts with aqueous silver nitrate to produce aqueous iron(iii) nitrate and silver metal. IDENTIFY THE TYPE OF REACTION, PREDICT THE PRODUCTS (STATES NOT REQUIRED), AND BALANCE THE EQUATION: 11. Al(s) + NaOH(aq) 12. C 2 H 4 (g) + O 2 (g) 13. FeCl 2 (aq)+ K 2 S(aq) 14. Ba(s) + O 2 (g) 15. NH 4 NO 3 (aq) + NaCl(aq) 16. SO 2 (g) 17. Magnesium metal is added to aqueous hydrochloric acid. 18. Potassium metal is combined with chlorine gas. 19. Aqueous solutions of potassium bromide and silver nitrate are combined.

5 Chemical Reactions Review ANSWER KEY 1. synthesis 2Sb + 3I 2 2SbI 3 2. single replacement 2Li + 2H 2 O 2LiOH + H 2 3. decomposition 2AlCl 3 2Al + 3Cl 2 4. combustion C 6 H O 2 6CO 2 + 6H 2 O 5. double replacement 2AlCl 3 + 3Na 2 CO 3 Al 2 (CO 3 ) 3 + 6NaCl 6. double replacement 2HNO 3 + Ba(OH) 2 Ba(NO 3 ) 2 + 2H 2 O 7. single replacement 2Al + 3Pb(NO 3 ) 2 2Al(NO 3 ) 3 + 3Pb 8. double replacement 2NH 4 Cl(aq) + Pb(NO 3 ) 2 (aq) PbCl 2 (s) + 2NH 4 NO 3 (aq) 9. combustion CS 2 (s) + 3O 2 (g) CO 2 (g) + 2SO 2 (g) 10. single replacement Fe(s) + 3AgNO 3 (aq) Fe(NO 3 ) 3 (aq) + 3Ag(s) 11. single replacement Al(s) + NaOH(aq) N.R. 12. combustion C 2 H 4 (g)+ 3O 2 (g) 2CO 2 (g) + 2H 2 O(g) 13. double replacement FeCl 2 (aq)+ K 2 S(aq) FeS(s) + 2KCl(aq) 14. comb, synthesis 2Ba(s) + O 2 (g) 2BaO(s) 15. double replacement NH 4 NO 3 (aq) + NaCl(aq) N.R. 16. decomposition SO 2 (g) S(s) + O 2 (g) 17. single replacement Mg(s) + 2HCl(aq) MgCl 2 (aq) + H 2 (g) 18. synthesis 2K(s) + Cl 2 (g) 2KCl(s) 19. double replacement KBr(aq) + AgNO 3 (aq) AgBr(s) + KNO 3 (aq)