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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) 23C to K 1.25 x 10-1 Kg 2) 21.3 Km to cm 2.13 x 10 6 cm 2.69 x 10 3 cm 3 7) 18.2 ml to cm x 10 1 ml 1.8 x 10-3 cm 3 12) 2.45 L to µm x10 15 µm 2.2 Kg 17) 1.2 m to inches 47.9 " 296 K 22) 180 C to K 453 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) 540K to C 3.34 x 10-1 cm 7.28 x 10-7 m 4.04 x 10 6 cm 6.03 x 10 1 lb 267 C 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 C 1.23 x 10-3 L 5) 47.5 cm 3 to L 4.75 x 10-2 L Scientific Notation 8.32 x 10 1 mg 10) Mg to dg x 10 7 dg 8.98 x 10-3 g 15) 50.1 mm to Km 5.01 x 10-5 Km 1.14 x 10 2 g 20) 6'4" to cm 190 cm 4727C 25) 27C to K 300 K 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 ]= 7) [ 2.3 x ]= [1.64 x ] [4.17 x 10 9 ] 6.0 x ) [27.3 x ][2.0 x ]= x )[ 4.2 x ][9.4 x 10 7 ]= [6.4 x 10 9 ] 6.2 x x ) [ x 10 2 ][ x ]= 3.6 x ) [ 1.7 x 10 9 ][3.9 x 10 7 ]= [1.40 x 10-6 ] 4.7 x ) [ 4.50 x 10 9 ]= [6.636 x ] 6.78 x )[7.4 x 10 6 ][1.9 x 10-3 ] = [5.3 x 10 6 ][1.7 x 10-8 ][2.4x 10 5 ] 3.0 Density Problems 1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3? v = 2.38 x 10 7 cm 3 1

2 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? m = 3.75 x 10 4 g 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)? 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? g/mol 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? g/mol 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? g/mol 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: CuCl 2 + 2NaNO 3 Cu(NO 3 ) 2 + 2NaCl ( 2 If 15 grams of copper (II) chloride react with 20 grams of sodium nitrate, how much sodium chloride can be formed? 13 g ( 3 What is the limiting reagent for the reaction in #2? copper (II) chloride ( 4 How much of the nonlimiting reagent is left over in this reaction? 0.88 g 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? 86.9% 2

3 Mole Problems Molecular Mass / Formula Mass 1) Find the formula mass of KMnO 4. Total g 2) Find the formula mass of Mg 3 (PO 4 ) 2. Total g 3) Find the molecular mass of C 12 H 22 O 11. Total g 1) How many moles are in 17.7 g of KMnO 4? mol KMnO 4 How many formula units are in 17.7 g KMnO 4? x formula units KMnO 4 How many atoms of O are in 17.7 g KMnO 4? 2.70 x atoms O 2) How many moles are in 41.2 g of Mg 3 (PO 4 ) 2? 1.57 mol Mg 3 (PO 4 ) 2 How many formula units are in 41.2 g Mg 3 (PO 4 ) 2? 9.44 x units Mg 3 (PO 4 ) 2 How many atoms of P are in 41.2 g Mg 3 (PO 4 ) 2? 1.89 x atoms P 3) How many moles are in 26.9 g of C 12 H 22 O 11? mol C 12 H 22 O 11 How many molecules are in 26.9 g of C 12 H 22 O 11? 4.73 x molecules C 12 H 22 O 11 How many atoms of C are in 26.9 g of C 12 H 22 O 11? 5.68 x atoms C 4) How many moles are 19.8 x molecules C 12 H 22 O 11? 32.9 mol C 12 H 22 O 11 What is the mass of 19.8 x molecules C 12 H 22 O 11? 1.13x10 4 g 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? 5.73 x mol Mg 3 (PO 4 ) 2 6) How many moles of KMnO 4 are 3.64 x atoms of Mn in KMnO 4? 60.6 mol KMnO 4 3

4 Percent Composition 1) Find the percentage composition of KMnO % K 34.77% Mn 40.48% O 2) Find the percentage composition of Mg 3 (PO 4 ) % Mg 23.57% P 48.68% Mg 3) Find the percentage composition of C 12 H 22 O % C 6.49% H 51.40% C Empirical Formula 1) What is the empirical formula for a compound if a 83.7 g sample contains 44.28g Al and g O? Al 2 O 3 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? CH 2 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? CH 2 O empirical formula C 6 H 12 O 6 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? NO empirical formula N 2 O 2 molecular formula 4

5 Balancing Chemical Equations Predict the products and write the balanced equation for the reactions. 1. Mg + 2AgNO 3 --> 2Ag + Mg(NO 3 ) 2 2. Ba + H 2 SO 4 --> H 2 + BaSO 4 3. CaCl 2 + 2NaOH --> 2NaCl + Ca(OH) 2 4. O 2 + 2H 2 --> 2H 2 O 5. SiO 2 -- > Si + O 2 Write balanced equations for each of the following reactions. 1.) 4Fe + 3O 2 -> 2Fe 2 O 3 2.) 2KClO 3 -> 2KCl + 3O 2 3.) Ca(OH) 2 + H 2 SO 4 -> 2HOH + CaSO 4 4.) 2HgO -> 2Hg + O 2 5.) Cu + 2AgNO 3 -> Cu(NO 3 ) 2 + 2Ag 6.) 2C 4 H O 2 --> 8CO H 2 O 7.) C 9 H O 2 --> 9CO H 2 O 8.) CrCl 3 + NaOH--> Cr 2 O 3 + HCl + NaCl 9.) 2NaClO 3 --> 2NaCl + 3O 2 10.) C 23 H O 2 --> 23CO H 2 O 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._3_ Ba(OH) 2 + _2_H 3 PO 4 _1_Ba3(PO 4 ) 2 + _6_ 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 2Na + Cl 2 --> 2NaCl 2.5 mol Cl 2 1b) Using the equation (after it is balanced) above, determine the amount of product that can be produced from 24.7 g Na. 62 g NaCl 1c) How many molecules of product would be produced from 24.7g Na? 6.5 E 23 NaCl molecules 2a) In the reaction 2C 8 H O 2 --> 16CO H 2 O, the ratio of volumes of O 2 to CO 2 is 25:16 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? 37.8 g H 2 O 1.15 E 24 molecules CO 2 2d) How many atoms of H are in 2 mol of C 8 H 18? 2.2 E 25 atoms H 2e) What is the percentage, by mass, of the H in 2 mol of C 8 H 18? 1.37 E 26 amu C 8 H E 25 amu H 16% H 6

7 Molarity Problems 1) How many grams of potassium carbonate are needed to make 200 ml of a 2.5 M solution? 69.1 grams 2) How many liters of 4 M solution can be made using 100 grams of lithium bromide? 3.47 L ( 3 What is the concentration of a 450 ml solution that contains 200 grams of iron (II) chloride? 3.51 M ( 4 How many grams of ammonium sulfate are needed to make a 0.25 M solution at a concentration of 6 M? g 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 0.85 M 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? M=0.19M 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? M 7

8 1) Which of the following compounds is likely soluble in water? Compound soluble Insoluble Fe(NO 3 ) 3 AgCl Look at solubility rules to answer this question 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 (insoluble are in bold) 1) Pb(NO 3 ) 2 (aq) + 2KI (aq) PbI 2 (s) + 2 KNO 3 (aq)? 2) Mg(NO 3 ) 2 (aq) + 2NaOH (aq) Mg(OH) 2 (s) + 2NaNO 3 (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) Pb(NO 3 ) 2 (aq) + 2KI (aq) PbI 2 (s) + 2KNO 3 (aq) Pb 2+ (aq) + 2NO 3- (aq) + 2K + (aq) + 2I - (aq) PbI 2 (s) + 2K + (aq) + 2NO 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) + 3 KOH (aq) > K 3 PO 4 (aq) + 3 H 2 O What is the net ionic equation? Total ionic equation: (spectator ions are in bold) 3H + (aq) + PO 4 3- (aq) + 3K + (aq) + 3OH - (aq) 3K + (aq) + PO 4 3- (aq) + 3H 2 O (l) Net ionic 3H + (aq) + 3OH - (aq) 3H 2 O (l) 6) What is the net ionic equation for the reaction between Na 2 CO 3 (aq) and HCl(aq)? Na 2 CO 3 (aq) + 2 HCl (aq) 2 NaCl (aq) + H 2 O + CO 2 (g) Total Net ionic 2Na + (aq) + CO 3-2 (aq) + 2H + (aq) + 2Cl - (aq) 2Na + (aq) + 2Cl - (aq) + H 2 O(l) +CO 2 (g) Net ionic: CO 3 (-2) (aq) + 2H + (aq) -> H 2 O (l) + CO 2 (g) 7) Which of these reactions will react and give products? (Based on activity series) Fe + CuSO 4 Cu + Fe 2 (SO 4 ) 3 Ni + NaCl No reaction Li + ZnCO 3 Zn + Li 2 CO 3 Al + CuCl 2 Cu + AlCl 3 Mg + AgNO 3 Ag + Mg(NO 3 ) 2 Cu + AgNO 3 Ag + Cu(NO 3 ) 2 Mg + H 2 SO 4 H 2 + MgSO 4 Zn + AgNO 3 Ag + Zn(NO 3 ) 2 Cu + Fe(NO 3 ) 3 No reaction Cl 2 + 2KBr 2KCl + Br 2 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 S = +6 = oxidation number in H 2 SO 4 a. NaOH Na = _+1 ; O = -2_; H = +1 9

10 b. HCl H = _+1 ; Cl = _-1 c. N 2 O 3 N = _+3 ; O = -2_ d. CaC 2 O 4 Ca = _+2 ; C = _+3 ; O = _-2 e. SF 6 S = _+6 ; F = _-1 f. H 2 Se H = _+1 ; Se = _-2 g. H 2 O 2 H = _+1 ; O = _-1 Write the oxidation number of each atom in these ions: 2-1. SO S = _+6 ; O = -2_ 4 2. HPO NO 2 - H = _1+ N = +3 ; ; P = _+3 ; O = _-2 O = _-2 4. OH - O = _-2 ; H = _+1 5. HSO 4-6. HAsO 4 2- H = _+1 ; S = _+6 ; O = -2 H = _+1 ; As = _+5 ; O = -2 10

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