{"id":2243,"date":"2018-04-11T23:52:22","date_gmt":"2018-04-12T03:52:22","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/end-of-chapter-material-4\/"},"modified":"2019-06-20T13:54:00","modified_gmt":"2019-06-20T17:54:00","slug":"end-of-chapter-material-4","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/end-of-chapter-material-4\/","title":{"raw":"7.6 End of Chapter Problems","rendered":"7.6 End of Chapter Problems"},"content":{"raw":"
\r\n

1. How many molecules of O2<\/sub> will react with 6.022 \u00d7 1023<\/sup> molecules of H2<\/sub> to make water?<\/p>\r\n

The reaction is 2 H2<\/sub>(g) +\u00a0O2<\/sub>(g) $latex \\longrightarrow$<\/span><\/span><\/span> 2 H2<\/sub>O(\u2113).<\/p>\r\n

2. How many moles are present in 6.411 kg of CO2<\/sub>? How many molecules is this?<\/p>\r\n

3. What is the mass in milligrams of 7.22 \u00d7 1020<\/sup> molecules of CO2<\/sub>?<\/p>\r\n

4. What is the mass in grams of 1 molecule of H2<\/sub>O?<\/p>\r\n

5. What is the volume of 3.44 mol of Ga if the density of Ga is 6.08 g\/mL?<\/p>\r\n

6. For the chemical reaction<\/p>\r\n\r\n<\/div>\r\n

\r\n\r\n2 C4<\/sub>H10<\/sub>(g) +\u00a013 O2<\/sub>(g) $latex \\longrightarrow$<\/span>\u00a08 CO2<\/sub>(g) +\u00a010 H2<\/sub>O(\u2113)<\/span><\/span>\r\n

assume that 13.4 g of C4<\/sub>H10<\/sub> reacts completely to products. The density of CO2<\/sub> is 1.96 g\/L. What volume in liters of CO2<\/sub> is produced?<\/p>\r\n

7. Calculate the mass of each product when 100.0 g of CuCl react according to the reaction<\/p>\r\n\r\n<\/div>\r\n

\r\n\r\n2 CuCl(aq) $latex \\longrightarrow$<\/span>\u00a0CuCl2<\/sub>(aq) +\u00a0Cu(s)<\/span><\/span>\r\n

What do you notice about the sum of the masses of the products? What concept is being illustrated here?<\/p>\r\n

8. What mass of CO2<\/sub> is produced from the combustion of 1 gal of gasoline? The chemical formula of gasoline can be approximated as C8<\/sub>H18<\/sub>. Assume that there are 2,801 g of gasoline per gallon.<\/p>\r\n

9. A chemical reaction has a theoretical yield of 19.98 g and a percent yield of 88.40%. What is the actual yield?<\/p>\r\n

10. Given the initial amounts listed, what is the limiting reagent, and how much of the other reactants are in excess?<\/p>\r\n2 P4<\/sub> <\/span>+\u00a0 <\/span>6 NaOH +\u00a0 6 H2<\/sub>O\u00a0\u00a0$latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0 3 Na2<\/sub><\/span>HPO4<\/sub>\u00a0 <\/span>+\u00a0 5 P<\/span>H3<\/sub>\r\n\r\n<\/div>\r\n

\r\n\r\nInitial amounts used: P4\u00a0<\/sub>= 35.0 g;\u00a0NaOH = 12.7 g; H2<\/sub>O = 9.33 g\r\n\r\n11. Verify that it does not matter which product you use to predict the limiting reagent by using both products in this combustion reaction to determine the limiting reagent and the amount of the reactant in excess. Initial amounts of each reactant are given.\r\n\r\n<\/div>\r\n
\r\n\r\n\"Screen<\/a>\r\n

12. Chlorine can be produced by the reaction of hydrochloric acid with excess manganese(IV) oxide according to the following reaction: 4HCl(aq) + MnO2<\/sub>(s) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a0Cl2<\/sub>(g) + 2H2<\/sub>O(l) + MnCl2<\/sub>(aq). How many moles of HCl are needed to form 12.5 mol Cl2<\/sub>?<\/p>\r\n

13. How many moles of aluminum oxide will be produced by reacting 9.5 mol of Al with O2<\/sub>?\r\nHow many moles of O2<\/sub>will react?<\/p>\r\n

14. Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide:<\/p>\r\n

2NO(g) + O2<\/sub>(g) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a02NO2<\/sub>(g)\r\nStarting with 2.2 mol NO, how many moles and how many grams of O2\u00a0<\/sub>are required for complete reaction? What mass of NO2<\/sub>, in grams, is produced?<\/p>\r\n

15. How many grams of Mg will react with 7.5 grams of H2<\/sub>SO4\u00a0<\/sub>in the reaction:\r\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>Mg\u00a0<\/span>+\u00a0 <\/span>H2<\/sub>SO4<\/sub>\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>MgSO4<\/sub>\u00a0 <\/span>+\u00a0 <\/span>H2<\/sub><\/p>\r\n

16. Zinc will react with hydrochloric acid producing hydrogen gas and zinc chloride:\r\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>Zn\u00a0<\/span>+\u00a0 <\/span>2HCl\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>ZnCl2<\/sub>\u00a0 <\/span>+\u00a0 <\/span>H2<\/sub>\r\nHow many grams of H2\u00a0<\/sub>will be produced if 5.0 grams of zinc are used?<\/p>\r\n

17. The final step in the manufacture of platinum metal (for use in automotive catalytic converters and other products) is the reaction: 3(NH4<\/sub>)2<\/sub>PtCl6<\/sub>(s) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a03Pt(s) + 2NH4<\/sub>Cl(s) + 2N2<\/sub>(g) + 16HCl(g)\r\nHow many grams of Pt can be produced by decomposing 12.35 g (NH4<\/sub>)2<\/sub>PtCl6<\/sub>?<\/p>\r\n

18. How many kilograms of NH3\u00a0<\/sub>will be produced when 25.0 kg of H2\u00a0<\/sub>reacts with excess N2<\/sub>?<\/p>\r\n

19. A 3.00 cm3\u00a0<\/sup>piece of aluminum reacts with a solution of HCl and produces H2\u00a0<\/sub>gas and AlCl3<\/sub>. Determine the mass of H2\u00a0<\/sub>formed. (Al has a density of 2.70 g\/cm3<\/sup>)<\/p>\r\n

20. One of the most important commercial reactions is the \"Haber\" production of ammonia:\r\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>3H2<\/sub>(g)\u00a0 <\/span>+\u00a0 <\/span>N2<\/sub>(g)\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2NH3<\/sub>(g)\r\nChiefly by this reaction, the industrial \"fixation\" of nitrogen now accounts for about one-third of all the nitrogen fixed on our planet. If 3.0 kg of H2\u00a0<\/sub>and 1.0 kg of N2\u00a0<\/sub>are mixed and allowed to react until one or both of the reactants is used up,\r\na)\u00a0\u00a0 <\/span>how many moles of the NH3\u00a0<\/sub>molecules are produced?\r\nb)\u00a0\u00a0 <\/span>how many moles of the H2\u00a0<\/sub>are left?\r\nc)\u00a0\u00a0 <\/span>how many moles of the N2\u00a0<\/sub>are left?<\/p>\r\n

21. Iron reacts with chlorine to produce FeCl3\u00a0<\/sub>as:\u00a0 <\/span>2Fe\u00a0<\/span>+\u00a0 <\/span>3Cl2<\/sub>\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2FeCl3<\/sub>\r\nIf 10.6 grams of iron are mixed with 18.9 grams of chlorine and allowed to react,\r\na)\u00a0\u00a0 <\/span>how many grams of FeCl3\u00a0<\/sub>will be produced?<\/span>\r\nb)\u00a0\u00a0 <\/span>how many grams of excess reactant will be left after the reaction is complete?<\/p>\r\n

22. Silver tarnishes in the presence of hydrogen sulfide in the following reaction:\r\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>4Ag\u00a0 <\/span>+\u00a0 <\/span>2H2<\/sub>S\u00a0 <\/span>+\u00a0 <\/span>O2<\/sub>\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2Ag2<\/sub>S\u00a0 <\/span>+\u00a0 <\/span>2H2<\/sub>O\r\n<\/span>How many grams of Ag2<\/sub>S can be obtained by this reaction from a mixture of 0.950 g Ag, 0.140 g H2<\/sub>S, and 0.0800 g O2<\/sub>?<\/p>\r\n

23. 11.92 g of Pb(NO3<\/sub>)2\u00a0<\/sub>and 20.31 g of KI react as:\u00a0 <\/span>Pb(NO3<\/sub>)2<\/sub>+ 2 KI\u00a0 $latex \\longrightarrow$<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>PbI2<\/sub>\u00a0 <\/span>+\u00a0 <\/span>2 KNO3<\/sub>\r\nHow many grams of PbI2\u00a0<\/sub>are produced if the yield of the reaction is 81%?<\/p>\r\n

24. Reaction of H2\u00a0<\/sub>and N2\u00a0<\/sub>produces ammonia (NH3<\/sub>) with 65.5%yield. If 30.0 g of NH3\u00a0<\/sub>are required, how many grams of N2\u00a0<\/sub>and how many of H2\u00a0<\/sub>must be used?<\/p>\r\n

25. Solid calcium carbonate dissolves in a solution of hydrochloric acid and reacts to form a solution of calcium chloride and water, and bubbles of carbon dioxide.\r\n<\/span><\/p>\r\n

How many grams of calcium chloride will form if 40.0 g of CaCO3\u00a0<\/sub>is mixed with 0.500 mol of HCl?\r\nHow many grams of calcium carbonate, if any, will remain unreacted?<\/p>\r\n

26. Freon-12 (CCl2<\/sub>F2<\/sub>) is a gas that has been used as a refrigerant. It is prepared by the reaction between carbon tetrachloride and antimony trifluoride. The other product that is produced is SbCl3<\/sub>. If the percent yield is 72.0%, how many grams of antimony trifluoride must be treated with excess carbon tetrachloride to obtain an actual yield of 25.0 grams of Freon-12?<\/p>\r\n

27. Aluminum chloride (Al2<\/sub>Cl6<\/sub>) can be made by the following reaction: 2Al(s) + 3Cl2<\/sub>(g) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a0<\/span>Al2<\/sub>Cl6<\/sub>(s)\r\na)\u00a0 <\/span>which reactant is limiting if 2.70 g Al and 4.05 g Cl2\u00a0<\/sub>are mixed?\r\nb)\u00a0 <\/span>what mass of Al2<\/sub>Cl6\u00a0<\/sub>can be produced?\r\nc)\u00a0 <\/span>What mass of the excess reactant will remain when the reaction is complete?<\/p>\r\n

28. Iron oxide can be reduced to the metal as follows: Fe2<\/sub>O3<\/sub>(s) + 3CO(g) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a0<\/span>2Fe(s) + 3CO2<\/sub>(g)\r\nHow many grams of iron can be obtained from 1.00 kg of the iron oxide?\r\nIf 654 g Fe was obtained from the reaction, what was the percent yield?<\/p>\r\n

29. Disulfur dichloride can be prepared by the following reaction:\r\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>3SCl2<\/sub>(l) + 4NaF(s) $latex \\longrightarrow$<\/span><\/span><\/span>\u00a0<\/span>SF4<\/sub>(g) + S2<\/sub>Cl2<\/sub>(l) + 4NaCl(s)\r\nWhat mass of SCl2<\/sub>is needed to react with excess NaF to prepare 1.19 g S2<\/sub>Cl2<\/sub>, if the yield is 51%?<\/p>\r\n

30. You have a 0.12 M solution of BaCl2<\/sub>. What ions exist in the solution, and what are their concentrations?<\/p>\r\n

31. Assume that 6.73 g Na2<\/sub>CO3<\/sub>is dissolved in enough water to make 250. mL of solution,\r\na) what is the molarity of the sodium carbonate?\r\nb) What are the concentrations of the Na+<\/sup>and CO3<\/sub>2-<\/sup>ions?<\/p>\r\n

32. What is the mass, in grams, of solute in 250. mL of a 0.0125 M solution of KMnO4<\/sub>?<\/p>\r\n

33. What volume of 0.123 M NaOH, in mL, contains 25.0 g NaOH?<\/p>\r\n

34. What is the maximum mass, in grams, of AgCl that can be precipitated by mixing 50.0 mL 0.025 M AgNO3<\/sub>solution with 100.0 mL of 0.025 M NaCl solution? Which reactant is in excess? What is the concentration of the excess reactant remaining in solution after the AgCl has precipitated?<\/p>\r\n35. How many moles of NaOH react with 7.80 mol of the acid H2<\/sub>SO4<\/sub>?\r\n

36. How many mL of 0.512 M NaOH is required to react completely with 25.0 mL of 0.234 M H2<\/sub>SO4<\/sub>?<\/p>\r\n

37. What mass, in grams, of Na2<\/sub>CO3<\/sub>is required for complete reaction with 25.0 mL of 0.155 M HNO3<\/sub>? \u00a0\u00a0\u00a0\u00a0 <\/span>Na2<\/sub>CO3(aq)<\/sub>+ 2HNO3(aq)<\/sub> $latex \\longrightarrow$<\/span><\/span><\/span><\/span><\/span>\u00a0<\/sub><\/span>2NaNO3(aq)<\/sub>+ CO2(g)<\/sub>+ H2<\/sub>O(l)<\/sub><\/span><\/p>\r\n\r\n

<\/h2>\r\n

Answers<\/h2>\r\n1. 3.011 \u00d7 1023<\/sup> molecules of O2<\/sub>\r\n\r\n2. 145.7 mol; 8.77 \u00d7 1025<\/sup> molecules\r\n\r\n3.\u00a052.8 mg\r\n\r\n4.\u00a02.99 \u00d7 10\u221223<\/sup> g\r\n\r\n5.\u00a039.4 mL\r\n\r\n6.\u00a020.7 L\r\n\r\n7.\u00a067.91 g of CuCl2<\/sub>; 32.09 g of Cu. The two masses add to 100.0 g, the initial amount of starting material, demonstrating the law of conservation of matter.\r\n\r\n8.\u00a08633 g\r\n\r\n9.\u00a017.66 g\r\n\r\n10.\u00a0The limiting reagent is NaOH; 21.9 g of P4<\/sub> and 3.61 g of H2<\/sub>O are left over.\r\n\r\n11.\u00a0Both products predict that O2<\/sub> is the limiting reagent; 20.3 g of C3<\/sub>H8<\/sub> are left over.\r\n

12.\u00a0\u00a0 <\/span>50.0 mol HCl<\/span><\/p>\r\n

13.\u00a0\u00a0 <\/span>4.8 mol Al2<\/sub>O3<\/sub>\u00a0\u00a0\u00a0 <\/span>7.1 mol O2<\/sub><\/span><\/p>\r\n

14.\u00a0\u00a0 <\/span>1.1 mol O2<\/sub>\u00a0\u00a0\u00a0 <\/span>35 g O2<\/sub>\u00a0\u00a0\u00a0 <\/span>1.0 x 102<\/sup>g NO2<\/sub><\/span><\/p>\r\n

15.\u00a0\u00a0 <\/span>1.9 g Mg<\/span><\/p>\r\n

16.\u00a0 <\/span>0.15 g H2<\/sub><\/span><\/p>\r\n

17.\u00a0 <\/span>5.428 g Pt<\/span><\/p>\r\n

18.\u00a0 <\/span><\/span>141 kg NH3<\/sub><\/p>\r\n

19.\u00a0 <\/span>0.908 g H2<\/sub><\/span><\/p>\r\n

20.\u00a0 <\/span>71 mol NH3<\/sub>\u00a0\u00a0\u00a0 <\/span>1.4 x 103<\/sup>mol H2<\/sub>\u00a0\u00a0\u00a0 <\/span>0 mol N2<\/sub><\/span><\/p>\r\n

21.\u00a0 <\/span>28.8 g FeCl3<\/sub>\u00a0\u00a0\u00a0 <\/span>0.7 g Fe<\/span><\/p>\r\n

22.\u00a0 <\/span>1.02 g Ag2<\/sub>S<\/span><\/p>\r\n

23.\u00a0 <\/span>13 g PbI2<\/sub><\/span><\/p>\r\n

24.\u00a0 <\/span>37.7 g N2<\/sub>\u00a0\u00a0\u00a0 <\/span>8.13 g H2<\/sub><\/span><\/p>\r\n

25.\u00a0 Must use a balanced equation to solve this:<\/span><\/span><\/p>\r\n

1 CaCO3<\/sub>(s)\u00a0 +\u00a0 2 HCl(aq)\u00a0$latex \\longrightarrow$<\/span><\/span><\/span>\u00a01 CaCl2<\/sub>(aq) + 1 H2<\/sub>O(l) + 1 CO2<\/sub>(g)<\/span><\/span><\/p>\r\n

27.7g CaCl2<\/sub>\u00a0\u00a0\u00a0 <\/span>15.0g CaCO3\u00a0<\/sub>unreacted<\/span><\/p>\r\n

26.\u00a0 <\/span><\/span>34.2 g SbF3<\/sub><\/p>\r\n

27.\u00a0 <\/span>a) Cl2\u00a0<\/sub>is limiting\u00a0 <\/span>b) 5.08 g Al2<\/sub>Cl6<\/sub>\u00a0\u00a0 <\/span>c) 1.67 g Al unreacted<\/p>\r\n

28.\u00a0 <\/span><\/span>699 g\u00a0<\/span>93.5%<\/p>\r\n

29.\u00a0 <\/span>5.3 g SCl2<\/sub><\/span><\/p>\r\n

30.\u00a0 <\/span><\/span>0.12 M Ba2+<\/sup>, 0.24 M Cl-<\/sup><\/p>\r\n

31.\u00a0 <\/span>a) 0.254 M Na2<\/sub>CO3<\/sub>\u00a0\u00a0 <\/span>b) 0.508 M Na+<\/sup>, 0.254 M CO3<\/sub>2-<\/sup><\/span><\/p>\r\n

32.\u00a0 <\/span><\/span>0.494 g KMnO4<\/sub><\/span><\/p>\r\n

33.\u00a0 <\/span><\/span>5.08 x 103<\/sup>mL<\/span><\/p>\r\n

34.\u00a0 <\/span><\/span>0.18 g AgCl, NaCl, 0.0083 M NaCl<\/span><\/p>\r\n

35.\u00a0 <\/span><\/span>15.6 mol NaOH<\/p>\r\n

36.\u00a0 <\/span><\/span>22.9 mL NaOH solution<\/p>\r\n

37.\u00a0 <\/span><\/span>0.205 g Na2<\/sub>CO3<\/sub><\/p>\r\n\r\n<\/div>","rendered":"

\n

1. How many molecules of O2<\/sub> will react with 6.022 \u00d7 1023<\/sup> molecules of H2<\/sub> to make water?<\/p>\n

The reaction is 2 H2<\/sub>(g) +\u00a0O2<\/sub>(g) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span> 2 H2<\/sub>O(\u2113).<\/p>\n

2. How many moles are present in 6.411 kg of CO2<\/sub>? How many molecules is this?<\/p>\n

3. What is the mass in milligrams of 7.22 \u00d7 1020<\/sup> molecules of CO2<\/sub>?<\/p>\n

4. What is the mass in grams of 1 molecule of H2<\/sub>O?<\/p>\n

5. What is the volume of 3.44 mol of Ga if the density of Ga is 6.08 g\/mL?<\/p>\n

6. For the chemical reaction<\/p>\n<\/div>\n

\n

2 C4<\/sub>H10<\/sub>(g) +\u00a013 O2<\/sub>(g) [latex]\\longrightarrow[\/latex]<\/span>\u00a08 CO2<\/sub>(g) +\u00a010 H2<\/sub>O(\u2113)<\/span><\/span><\/p>\n

assume that 13.4 g of C4<\/sub>H10<\/sub> reacts completely to products. The density of CO2<\/sub> is 1.96 g\/L. What volume in liters of CO2<\/sub> is produced?<\/p>\n

7. Calculate the mass of each product when 100.0 g of CuCl react according to the reaction<\/p>\n<\/div>\n

\n

2 CuCl(aq) [latex]\\longrightarrow[\/latex]<\/span>\u00a0CuCl2<\/sub>(aq) +\u00a0Cu(s)<\/span><\/span><\/p>\n

What do you notice about the sum of the masses of the products? What concept is being illustrated here?<\/p>\n

8. What mass of CO2<\/sub> is produced from the combustion of 1 gal of gasoline? The chemical formula of gasoline can be approximated as C8<\/sub>H18<\/sub>. Assume that there are 2,801 g of gasoline per gallon.<\/p>\n

9. A chemical reaction has a theoretical yield of 19.98 g and a percent yield of 88.40%. What is the actual yield?<\/p>\n

10. Given the initial amounts listed, what is the limiting reagent, and how much of the other reactants are in excess?<\/p>\n

2 P4<\/sub> <\/span>+\u00a0 <\/span>6 NaOH +\u00a0 6 H2<\/sub>O\u00a0\u00a0[latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0 3 Na2<\/sub><\/span>HPO4<\/sub>\u00a0 <\/span>+\u00a0 5 P<\/span>H3<\/sub><\/p>\n<\/div>\n

\n

Initial amounts used: P4\u00a0<\/sub>= 35.0 g;\u00a0NaOH = 12.7 g; H2<\/sub>O = 9.33 g<\/p>\n

11. Verify that it does not matter which product you use to predict the limiting reagent by using both products in this combustion reaction to determine the limiting reagent and the amount of the reactant in excess. Initial amounts of each reactant are given.<\/p>\n<\/div>\n

\n

\"Screen<\/a><\/p>\n

12. Chlorine can be produced by the reaction of hydrochloric acid with excess manganese(IV) oxide according to the following reaction: 4HCl(aq) + MnO2<\/sub>(s) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a0Cl2<\/sub>(g) + 2H2<\/sub>O(l) + MnCl2<\/sub>(aq). How many moles of HCl are needed to form 12.5 mol Cl2<\/sub>?<\/p>\n

13. How many moles of aluminum oxide will be produced by reacting 9.5 mol of Al with O2<\/sub>?
\nHow many moles of O2<\/sub>will react?<\/p>\n

14. Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide:<\/p>\n

2NO(g) + O2<\/sub>(g) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a02NO2<\/sub>(g)
\nStarting with 2.2 mol NO, how many moles and how many grams of O2\u00a0<\/sub>are required for complete reaction? What mass of NO2<\/sub>, in grams, is produced?<\/p>\n

15. How many grams of Mg will react with 7.5 grams of H2<\/sub>SO4\u00a0<\/sub>in the reaction:
\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>Mg\u00a0<\/span>+\u00a0 <\/span>H2<\/sub>SO4<\/sub>\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>MgSO4<\/sub>\u00a0 <\/span>+\u00a0 <\/span>H2<\/sub><\/p>\n

16. Zinc will react with hydrochloric acid producing hydrogen gas and zinc chloride:
\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>Zn\u00a0<\/span>+\u00a0 <\/span>2HCl\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>ZnCl2<\/sub>\u00a0 <\/span>+\u00a0 <\/span>H2<\/sub>
\nHow many grams of H2\u00a0<\/sub>will be produced if 5.0 grams of zinc are used?<\/p>\n

17. The final step in the manufacture of platinum metal (for use in automotive catalytic converters and other products) is the reaction: 3(NH4<\/sub>)2<\/sub>PtCl6<\/sub>(s) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a03Pt(s) + 2NH4<\/sub>Cl(s) + 2N2<\/sub>(g) + 16HCl(g)
\nHow many grams of Pt can be produced by decomposing 12.35 g (NH4<\/sub>)2<\/sub>PtCl6<\/sub>?<\/p>\n

18. How many kilograms of NH3\u00a0<\/sub>will be produced when 25.0 kg of H2\u00a0<\/sub>reacts with excess N2<\/sub>?<\/p>\n

19. A 3.00 cm3\u00a0<\/sup>piece of aluminum reacts with a solution of HCl and produces H2\u00a0<\/sub>gas and AlCl3<\/sub>. Determine the mass of H2\u00a0<\/sub>formed. (Al has a density of 2.70 g\/cm3<\/sup>)<\/p>\n

20. One of the most important commercial reactions is the “Haber” production of ammonia:
\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>3H2<\/sub>(g)\u00a0 <\/span>+\u00a0 <\/span>N2<\/sub>(g)\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2NH3<\/sub>(g)
\nChiefly by this reaction, the industrial “fixation” of nitrogen now accounts for about one-third of all the nitrogen fixed on our planet. If 3.0 kg of H2\u00a0<\/sub>and 1.0 kg of N2\u00a0<\/sub>are mixed and allowed to react until one or both of the reactants is used up,
\na)\u00a0\u00a0 <\/span>how many moles of the NH3\u00a0<\/sub>molecules are produced?
\nb)\u00a0\u00a0 <\/span>how many moles of the H2\u00a0<\/sub>are left?
\nc)\u00a0\u00a0 <\/span>how many moles of the N2\u00a0<\/sub>are left?<\/p>\n

21. Iron reacts with chlorine to produce FeCl3\u00a0<\/sub>as:\u00a0 <\/span>2Fe\u00a0<\/span>+\u00a0 <\/span>3Cl2<\/sub>\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2FeCl3<\/sub>
\nIf 10.6 grams of iron are mixed with 18.9 grams of chlorine and allowed to react,
\na)\u00a0\u00a0 <\/span>how many grams of FeCl3\u00a0<\/sub>will be produced?<\/span>
\nb)\u00a0\u00a0 <\/span>how many grams of excess reactant will be left after the reaction is complete?<\/p>\n

22. Silver tarnishes in the presence of hydrogen sulfide in the following reaction:
\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>4Ag\u00a0 <\/span>+\u00a0 <\/span>2H2<\/sub>S\u00a0 <\/span>+\u00a0 <\/span>O2<\/sub>\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>2Ag2<\/sub>S\u00a0 <\/span>+\u00a0 <\/span>2H2<\/sub>O
\n<\/span>How many grams of Ag2<\/sub>S can be obtained by this reaction from a mixture of 0.950 g Ag, 0.140 g H2<\/sub>S, and 0.0800 g O2<\/sub>?<\/p>\n

23. 11.92 g of Pb(NO3<\/sub>)2\u00a0<\/sub>and 20.31 g of KI react as:\u00a0 <\/span>Pb(NO3<\/sub>)2<\/sub>+ 2 KI\u00a0 [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span>\u00a0\u00a0<\/span>PbI2<\/sub>\u00a0 <\/span>+\u00a0 <\/span>2 KNO3<\/sub>
\nHow many grams of PbI2\u00a0<\/sub>are produced if the yield of the reaction is 81%?<\/p>\n

24. Reaction of H2\u00a0<\/sub>and N2\u00a0<\/sub>produces ammonia (NH3<\/sub>) with 65.5%yield. If 30.0 g of NH3\u00a0<\/sub>are required, how many grams of N2\u00a0<\/sub>and how many of H2\u00a0<\/sub>must be used?<\/p>\n

25. Solid calcium carbonate dissolves in a solution of hydrochloric acid and reacts to form a solution of calcium chloride and water, and bubbles of carbon dioxide.
\n<\/span><\/p>\n

How many grams of calcium chloride will form if 40.0 g of CaCO3\u00a0<\/sub>is mixed with 0.500 mol of HCl?
\nHow many grams of calcium carbonate, if any, will remain unreacted?<\/p>\n

26. Freon-12 (CCl2<\/sub>F2<\/sub>) is a gas that has been used as a refrigerant. It is prepared by the reaction between carbon tetrachloride and antimony trifluoride. The other product that is produced is SbCl3<\/sub>. If the percent yield is 72.0%, how many grams of antimony trifluoride must be treated with excess carbon tetrachloride to obtain an actual yield of 25.0 grams of Freon-12?<\/p>\n

27. Aluminum chloride (Al2<\/sub>Cl6<\/sub>) can be made by the following reaction: 2Al(s) + 3Cl2<\/sub>(g) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a0<\/span>Al2<\/sub>Cl6<\/sub>(s)
\na)\u00a0 <\/span>which reactant is limiting if 2.70 g Al and 4.05 g Cl2\u00a0<\/sub>are mixed?
\nb)\u00a0 <\/span>what mass of Al2<\/sub>Cl6\u00a0<\/sub>can be produced?
\nc)\u00a0 <\/span>What mass of the excess reactant will remain when the reaction is complete?<\/p>\n

28. Iron oxide can be reduced to the metal as follows: Fe2<\/sub>O3<\/sub>(s) + 3CO(g) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a0<\/span>2Fe(s) + 3CO2<\/sub>(g)
\nHow many grams of iron can be obtained from 1.00 kg of the iron oxide?
\nIf 654 g Fe was obtained from the reaction, what was the percent yield?<\/p>\n

29. Disulfur dichloride can be prepared by the following reaction:
\n\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>3SCl2<\/sub>(l) + 4NaF(s) [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a0<\/span>SF4<\/sub>(g) + S2<\/sub>Cl2<\/sub>(l) + 4NaCl(s)
\nWhat mass of SCl2<\/sub>is needed to react with excess NaF to prepare 1.19 g S2<\/sub>Cl2<\/sub>, if the yield is 51%?<\/p>\n

30. You have a 0.12 M solution of BaCl2<\/sub>. What ions exist in the solution, and what are their concentrations?<\/p>\n

31. Assume that 6.73 g Na2<\/sub>CO3<\/sub>is dissolved in enough water to make 250. mL of solution,
\na) what is the molarity of the sodium carbonate?
\nb) What are the concentrations of the Na+<\/sup>and CO3<\/sub>2-<\/sup>ions?<\/p>\n

32. What is the mass, in grams, of solute in 250. mL of a 0.0125 M solution of KMnO4<\/sub>?<\/p>\n

33. What volume of 0.123 M NaOH, in mL, contains 25.0 g NaOH?<\/p>\n

34. What is the maximum mass, in grams, of AgCl that can be precipitated by mixing 50.0 mL 0.025 M AgNO3<\/sub>solution with 100.0 mL of 0.025 M NaCl solution? Which reactant is in excess? What is the concentration of the excess reactant remaining in solution after the AgCl has precipitated?<\/p>\n

35. How many moles of NaOH react with 7.80 mol of the acid H2<\/sub>SO4<\/sub>?<\/p>\n

36. How many mL of 0.512 M NaOH is required to react completely with 25.0 mL of 0.234 M H2<\/sub>SO4<\/sub>?<\/p>\n

37. What mass, in grams, of Na2<\/sub>CO3<\/sub>is required for complete reaction with 25.0 mL of 0.155 M HNO3<\/sub>? \u00a0\u00a0\u00a0\u00a0 <\/span>Na2<\/sub>CO3(aq)<\/sub>+ 2HNO3(aq)<\/sub> [latex]\\longrightarrow[\/latex]<\/span><\/span><\/span><\/span><\/span>\u00a0<\/sub><\/span>2NaNO3(aq)<\/sub>+ CO2(g)<\/sub>+ H2<\/sub>O(l)<\/sub><\/span><\/p>\n

<\/h2>\n

Answers<\/h2>\n

1. 3.011 \u00d7 1023<\/sup> molecules of O2<\/sub><\/p>\n

2. 145.7 mol; 8.77 \u00d7 1025<\/sup> molecules<\/p>\n

3.\u00a052.8 mg<\/p>\n

4.\u00a02.99 \u00d7 10\u221223<\/sup> g<\/p>\n

5.\u00a039.4 mL<\/p>\n

6.\u00a020.7 L<\/p>\n

7.\u00a067.91 g of CuCl2<\/sub>; 32.09 g of Cu. The two masses add to 100.0 g, the initial amount of starting material, demonstrating the law of conservation of matter.<\/p>\n

8.\u00a08633 g<\/p>\n

9.\u00a017.66 g<\/p>\n

10.\u00a0The limiting reagent is NaOH; 21.9 g of P4<\/sub> and 3.61 g of H2<\/sub>O are left over.<\/p>\n

11.\u00a0Both products predict that O2<\/sub> is the limiting reagent; 20.3 g of C3<\/sub>H8<\/sub> are left over.<\/p>\n

12.\u00a0\u00a0 <\/span>50.0 mol HCl<\/span><\/p>\n

13.\u00a0\u00a0 <\/span>4.8 mol Al2<\/sub>O3<\/sub>\u00a0\u00a0\u00a0 <\/span>7.1 mol O2<\/sub><\/span><\/p>\n

14.\u00a0\u00a0 <\/span>1.1 mol O2<\/sub>\u00a0\u00a0\u00a0 <\/span>35 g O2<\/sub>\u00a0\u00a0\u00a0 <\/span>1.0 x 102<\/sup>g NO2<\/sub><\/span><\/p>\n

15.\u00a0\u00a0 <\/span>1.9 g Mg<\/span><\/p>\n

16.\u00a0 <\/span>0.15 g H2<\/sub><\/span><\/p>\n

17.\u00a0 <\/span>5.428 g Pt<\/span><\/p>\n

18.\u00a0 <\/span><\/span>141 kg NH3<\/sub><\/p>\n

19.\u00a0 <\/span>0.908 g H2<\/sub><\/span><\/p>\n

20.\u00a0 <\/span>71 mol NH3<\/sub>\u00a0\u00a0\u00a0 <\/span>1.4 x 103<\/sup>mol H2<\/sub>\u00a0\u00a0\u00a0 <\/span>0 mol N2<\/sub><\/span><\/p>\n

21.\u00a0 <\/span>28.8 g FeCl3<\/sub>\u00a0\u00a0\u00a0 <\/span>0.7 g Fe<\/span><\/p>\n

22.\u00a0 <\/span>1.02 g Ag2<\/sub>S<\/span><\/p>\n

23.\u00a0 <\/span>13 g PbI2<\/sub><\/span><\/p>\n

24.\u00a0 <\/span>37.7 g N2<\/sub>\u00a0\u00a0\u00a0 <\/span>8.13 g H2<\/sub><\/span><\/p>\n

25.\u00a0 Must use a balanced equation to solve this:<\/span><\/span><\/p>\n

1 CaCO3<\/sub>(s)\u00a0 +\u00a0 2 HCl(aq)\u00a0[latex]\\longrightarrow[\/latex]<\/span><\/span><\/span>\u00a01 CaCl2<\/sub>(aq) + 1 H2<\/sub>O(l) + 1 CO2<\/sub>(g)<\/span><\/span><\/p>\n

27.7g CaCl2<\/sub>\u00a0\u00a0\u00a0 <\/span>15.0g CaCO3\u00a0<\/sub>unreacted<\/span><\/p>\n

26.\u00a0 <\/span><\/span>34.2 g SbF3<\/sub><\/p>\n

27.\u00a0 <\/span>a) Cl2\u00a0<\/sub>is limiting\u00a0 <\/span>b) 5.08 g Al2<\/sub>Cl6<\/sub>\u00a0\u00a0 <\/span>c) 1.67 g Al unreacted<\/p>\n

28.\u00a0 <\/span><\/span>699 g\u00a0<\/span>93.5%<\/p>\n

29.\u00a0 <\/span>5.3 g SCl2<\/sub><\/span><\/p>\n

30.\u00a0 <\/span><\/span>0.12 M Ba2+<\/sup>, 0.24 M Cl–<\/sup><\/p>\n

31.\u00a0 <\/span>a) 0.254 M Na2<\/sub>CO3<\/sub>\u00a0\u00a0 <\/span>b) 0.508 M Na+<\/sup>, 0.254 M CO3<\/sub>2-<\/sup><\/span><\/p>\n

32.\u00a0 <\/span><\/span>0.494 g KMnO4<\/sub><\/span><\/p>\n

33.\u00a0 <\/span><\/span>5.08 x 103<\/sup>mL<\/span><\/p>\n

34.\u00a0 <\/span><\/span>0.18 g AgCl, NaCl, 0.0083 M NaCl<\/span><\/p>\n

35.\u00a0 <\/span><\/span>15.6 mol NaOH<\/p>\n

36.\u00a0 <\/span><\/span>22.9 mL NaOH solution<\/p>\n

37.\u00a0 <\/span><\/span>0.205 g Na2<\/sub>CO3<\/sub><\/p>\n<\/div>\n","protected":false},"author":330,"menu_order":7,"template":"","meta":{"pb_show_title":"on","pb_short_title":"7.6 End of Chapter Problems","pb_subtitle":"","pb_authors":[],"pb_section_license":"cc-by-nc-sa"},"chapter-type":[],"contributor":[],"license":[54],"class_list":["post-2243","chapter","type-chapter","status-publish","hentry","license-cc-by-nc-sa"],"part":1405,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2243","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/users\/330"}],"version-history":[{"count":13,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2243\/revisions"}],"predecessor-version":[{"id":4922,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2243\/revisions\/4922"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/parts\/1405"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2243\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/media?parent=2243"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapter-type?post=2243"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/contributor?post=2243"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/license?post=2243"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}