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

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1 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 3) 3.34 mm to cm 8) 728 nm to m 13) 40.4 Km to cm 18) 27.4 Kg to lb 23) 540F to ºC 4) 1.23 ml to L 9) 8.32 cg to mg 14) 8.98 mg to g 19) 0.25 lb to g 24) 5000K to ºC 5) 47.5 cm 3 to L 10) Mg to dg 15) 50.1 mm to Km 20) 6'4" to cm 25) 27ºC to F 2) Scientific Notation Complete the following calculations and express the answers in scientific notation. 1) [3.0 x 10-3 ][2.0 x 10 5 ]= 4)[ 4.6 x 10 1 ][2.1 x 10-4 ]= [1.64 x ] 7) [ 2.3 x ]= [4.17 x 10 9 ] 2) [27.3 x ][2.0 x ]= 5)[ 4.2 x ][9.4 x 10 7 ]= [6.4 x 10 9 ] 8) [ x 10 2 ][ x ]= 3) [ 1.7 x 10 9 ][3.9 x 10 7 ]= [1.40 x 10-6 ] 6) [ 4.50 x 10 9 ]= [6.636 x ] 9)[7.4 x 10 6 ][1.9 x 10-3 ] = [5.3 x 10 6 ][1.7 x 10-8 ][2.4x 10 5 ] Density Problems 1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3? 3) CaCl 2 is used as a de-icer on roads in the winter. It has a density of 2.50 g/cm 3. What is the mass of 15.0 L this substance? 1

2 1. What is average atomic mass of Lithium if 7.42% exists as 6Li (6.015 g/mol) and 92.58% exists as 7Li (7.016 g/mol)? 2. Magnesium has three naturally occuring isotopes % of Magnesium atoms exist as Magnesium-24 ( g/mol), 10.03% exist as Magnesium-25 ( g/mol) and 11.17% exist as Magnesium-26 ( g/mol). What is the average atomic mass of Magnesium? 3. Neon has two major isotopes, Neon-20 and Neon-22. Out of every 250 neon atoms, 225 will be Neon-20 ( g/mol), and 25 will be Neon-22 ( g/mol). What is the average atomic mass of Neon? 4. In a sample of 200 Chlorine atoms, it is found that 151 are 35 Cl ( g/mol), and 49 are 37 Cl ( g/mol). What is the average atomic mass of Chlorine? 5) When copper (II) chloride reacts with sodium nitrate, copper (II) nitrate and sodium chloride are formed. ( 1 Write the balanced equation for the reaction given above: ( 2 If 15 grams of copper (II) chloride react with 20 grams of sodium nitrate, how much sodium chloride can be formed? ( 3 What is the limiting reagent for the reaction in #2? ( 4 How much of the nonlimiting reagent is left over in this reaction? ( 5 If 11.3 grams of sodium chloride are formed in the reaction described in problem #2, what is the percent yield of this reaction? 2

3 Mole Problems Molecular Mass / Formula Mass 1) Find the formula mass of KMnO 4. 2) Find the formula mass of Mg 3 (PO 4 ) 2. 3) Find the molecular mass of C 12 H 22 O 11. Conversion of Moles, Grams, Molecules, and Atoms 1) How many moles are in 17.7 g of KMnO 4? How many formula units are in 17.7 g KMnO 4? How many atoms of O are in 17.7 g KMnO 4? 2) How many moles are in 41.2 g of Mg 3 (PO 4 ) 2? How many formula units are in 41.2 g Mg 3 (PO 4 ) 2? How many atoms of P are in 41.2 g Mg 3 (PO 4 ) 2? 3) How many moles are in 26.9 g of C 12 H 22 O 11? How many molecules are in 26.9 g of C 12 H 22 O 11? How many atoms of C are in 26.9 g of C 12 H 22 O 11? 4) How many moles are 19.8 x molecules C 12 H 22 O 11? What is the mass of 19.8 x molecules C 12 H 22 O 11? 5) How many moles of Mg 3 (PO 4 ) 2 are 27.6 x atoms of O in Mg 3 (PO 4 ) 2? 6) How many moles of KMnO 4 are 3.64 x atoms of Mn in KMnO 4? 3

4 Percent Composition 1) Find the percentage composition of KMnO 4. 2) Find the percentage composition of Mg 3 (PO 4 ) 2. 3) Find the percentage composition of C 12 H 22 O 11. Empirical Formula 1) What is the empirical formula for a compound if a 83.7 g sample contains 44.28g Al and g O? 2) What is the empirical formula for a compound if a 55.0 g sample contains 22.0 g C, 3.67 g H, and g O? Molecular Formula 1) A compound has a percentage composition of 40.01% C, 6.69 % H, and 53.30% O. Its molecular mass is amu. What is it's empirical formula? What is it's molecular formula? 2) A compound has a percentage composition of 46.68% N and 53.32% O. Its molecular mass is amu. What is the empirical formula? What is it's molecular formula? 4

5 Balancing Chemical Equations Predict the products and write the balanced equation for the reactions. 1. Mg + AgNO 3 --> 2. Ba + H 2 SO 4 --> 3. CaCl 2 + NaOH --> 4. O 2 + H 2 --> 5. SiO 2 -- > Write balanced equations for each of the following reactions. 1.) Fe + O 2 -> Fe 2 O 3 2.) KClO 3 -> KCl + O 2 3.) Ca(OH) 2 + H 2 SO 4 -> HOH + CaSO 4 4.) HgO -> Hg + O 2 5.) Cu + AgNO 3 -> Cu(NO 3 ) 2 + Ag 6.) C 4 H 10 + O 2 --> 7.) C 9 H 20 + O 2 --> 8.) CrCl 3 + NaOH--> Cr 2 O 3 + HCl + NaCl 9.) NaClO 3 --> NaCl + O 2 10.) C 23 H 48 + O 2 --> 1) Select the correct group of coefficients for the following neutralization equations A. HCl + Al(OH) 3 AlCl 3 + H 2 O a) 1,3,3, 1 b) 1,1,1, 3 c) 3,1,1,3 B. Ba(OH) 2 + H 3 PO 4 Ba3(PO 4 ) 2 + H 2 O a) 2,2,2,3 b) 6,1,3,3 c) 6,1,3, 2 5

6 Stoichiometry Problems 1a) How many moles of chlorine gas (Cl 2 ) would react with 5 moles of sodium (Na) according to the following chemical equation? (Balance equation.) Na + Cl 2 --> NaCl 1b) Using the equation (after it is balanced) above, determine the amount of product that can be produced from 24.7 g Na. 1c) How many molecules of product would be produced from 24.7g Na? 2a) In the reaction 2C 8 H O 2 --> 16CO H 2 O, the ratio of volumes of O 2 to CO 2 is 2b) If 27.3g of C 8 H 18 are combusted, what mass of water will be produced? 2c) How many molecules of CO 2 will be produced? 2d) How many atoms of H are in 2 mol of C 8 H 18? 2e) What is the percentage, by mass, of the H in 2 mol of C 8 H 18? 6

7 Molarity Problems 1) How many grams of potassium carbonate are needed to make 200 ml of a 2.5 M solution? 2) How many liters of 4 M solution can be made using 100 grams of lithium bromide? ( 3 What is the concentration of a 450 ml solution that contains 200 grams of iron (II) chloride? ( 4 How many grams of ammonium sulfate are needed to make a 0.25 M solution at a concentration of 6 M? 5) What is the concentration of a solution that has a volume of 2.5 L and contains 660 grams of calcium phosphate? Dilutions problems 1) If I have 340 ml of a 0.5 M NaBr solution, what will the concentration be if you add 560 ml more water to it? 2) If I dilute 250 ml of 0.10 M lithium acetate solution to a volume of 750 ml, what will the concentration of this solution be? 7

8 1) Which of the following compounds is likely soluble in water? Compound soluble Insoluble Fe(NO 3 ) 3 AgCl CaCO 3 (NH 4 ) 2 SO 4 CuSO 4 Cu(OH) 2 2) Complete the following equations and determine whether or not a precipitation reaction (exchange reaction) will occur. If a reaction will occur, balance the equation and 1) Determine the products of exchange reaction 2) Determine if there is any insoluble product 3) Balance the chemical equation 1) Pb(NO 3 ) 2 (aq) + KI (aq) 2) Mg(NO3)2 (aq) + KCl (aq) 3) Balance the following chemical equation and write the (complete) Ionic equation And the net Ionic equation and then determine the spectator ions 1) Pb(NO 3 ) 2 (aq) + KI (aq) PbI 2 (s) + KNO 3 (aq) 4) Write the net ionic equation for the precipitation reaction that may occur when solutions of calcium nitrate Ca(NO 3 ) 2 and sodium acetate (CH 3 COONa) are mixed. Write the balanced molecular equation, Check the solubility of products and determine the spectator ions 8

9 5) Complete and balance the following equation for an acid-base neutralization reaction: H 3 PO 4 (aq) + KOH(aq) What is the net ionic equation? 6) What is the net ionic equation for the reaction between Na 2 CO 3 (aq) and HCl(aq)? 7) Which of these reactions will react and give products? (Based on activity series) Fe + CuSO 4 Ni + NaCl Li + ZnCO 3 Al + CuCl 2 Mg + AgNO 3 Cu + AgNO 3 Mg + H 2 SO 4 Zn + AgNO 3 Cu + Fe(NO 3 ) 3 Cl 2 + 2KBr oxidation number 1) In H 2 SO 4 (sulfuric acid), calculate the oxidation number of the Sulfur atom? Write the oxidation number of each atom a. NaOH Na = ; O = ; H = b. HCl H = ; Cl = c. N 2 O 3 N = ; O = d. CaC 2 O 4 Ca = ; C = ; O = e. SF 6 S = ; F = f. H 2 Se H = ; Se = g. H 2 O 2 H = ; O = 9

10 Write the oxidation number of each atom in these ions: 2-1. SO S = ; O = 4 2. HPO NO 2 - H = N = ; ; P = ; O = O = 4. OH - O = ; H = 5. HSO 4 - H = ; S = ; O = 6. HAsO 4 2- H = ; As = ; O = 10