Final_Exam_worksheet.pdf

Final Exam Worksheet ? Chemistry 100-403, Spring 2010 The fourth exam and the final exam are cumulative and this worksheet just includes problems covering the contents taught after the 3rd exam. You will find practice for single displacement reactions in the worksheet for exam 3. Use worksheet Exam 1, Exam 2, and Exam 3 for additional practice. Chapter 5: Chemical Reactions 1. What is the balanced net ionic equation for the combination in aqueous solution? If no reaction occurs, write no reaction. a. Lead(II) acetate and sodium bromide b. Lithium phosphate and calcium sulfide c. Potassium chloride and barium hydroxide d. Ammonium carbonate and iron(III) iodide e. Cobalt(III) nitrate and barium sulfate f. Cesium nitrate and silver sulfate g. Calcium chloride and ammonium sulfate h. Lithium hydroxide and aluminum sulfate i. Silver sulfate and barium chloride Chapter 6: Stoichiometry 2. Use the balanced chemical reaction, to calculate the amounts listed. ( ) ( ) ( ) ( )3 2 2 24NH g 7O g 4NO g 6H O g+ ? + a. The mass of NO2 and water produced from 15.0 g of oxygen. b. The mass of NO2 and water produced from 15.0 moles of oxygen. c. The mass of NO2 and water produced from 15.0 g of ammonia. d. The mass of NO2 and water produced from 15.0 moles of ammonia. e. The mass of ammonia and oxygen required to produce 15.0 g of water. f. The mass of ammonia and oxygen required to produce 15.0 moles of water. g. The mass of ammonia and oxygen required to produce 15.0 g of NO2. h. The mass of ammonia and oxygen required to produce 15.0 moles of NO2. i. The number of oxygen molecules reacted from 0.1506 g of water. j. The number of ammonia molecules reacted from 150.6 g of water. k. The number of oxygen atoms reacted from 1.45 moles of NO2. l. The number of water molecules produced from 100 billion oxygen atoms. m. The total number of oxygen atoms produced from 1.30 g of oxygen. n. The mass of ammonia reacted when 9.8 × 1018 molecules of water are produced. 3. Based on the balanced chemical reaction, determine the limiting reactant and theoretical yield of water (in g). ( ) ( ) ( ) ( ) ( )2 5 2 2 2 2 24C H NO s 9O g 8CO g 10H O l 2N g+ ? + + a. Combine 45.0 g of both glycine (C2H5NO2) and oxygen. b. Combine 45.0 g of glycine and 35.0 g of oxygen. c. Combine 35.0 g of glycine and 45.0 g of oxygen. d. Combine 450 g of glycine and 45.0 g of oxygen. e. Combine 200.35 g of glycine and 45.0 g of oxygen. f. Combine 4500 mg of glycine and 1.25 g of oxygen. g. Combine 0.456 mg of glycine and 98.5 µg of oxygen. 4. Give the experimental yield of water for each combination in number 3 if the percent yield is 48.75%. 5. Give the experimental yield of water for each combination in number 3 if the percent yield is 98.75%. 6. Give the percent yield of water (using the information you calculated in number 3) for the experimental yields listed. a. 2.245 g of water b. 2.875 g of water c. 1.008 g of water d. 19.45 g of water e. 15.98 g of water f. 400 mg of water g. 25.5 µg of water. 7. Using the percent yields determined in number 6, determine the experimentally expected mass of water when each reaction is run with 43.56 mg of glycine in excess oxygen. 8. Based on the balanced net ionic equation, determine the desired quantity. ( ) ( ) ( ) ( )3+ 2-3 2 3 32Cr 3CO Cr COaq aq s+ ? a. Combine 15.0 mL of 0.125 M chromium (III) nitrate and 15.0 mL of 0.125 M ammonium carbonate. a. What is the limiting reactant? b. What is the theoretical yield in mass of chromium (III) carbonate? c. What is the experimental yield if the percent yield is 62.5%? d. If the reaction is run again with 25.5 mL of 0.255 M of chromium (III) nitrate and excess ammonium carbonate with a percent yield of 32.5%, what mass of chromium (III) carbonate will experimentally be recovered? b. Combine 75.5 mL of 0.505 M chromium (III) nitrate and 80.5 mL of 0.655 M ammonium carbonate. a. What is the limiting reactant? b. What is the theoretical yield in mass of chromium (III) carbonate? c. What is the experimental yield if the percent yield is 62.5%? c. Combine 75.5 mL of 0.505 M chromium (III) acetate and 80.5 mL of 0.655 M potassium carbonate. a. What is the limiting reactant? b. What is the theoretical yield in mass of chromium (III) carbonate? c. What is the experimental yield if the percent yield is 62.5%? d. Combine 10.55 mL of 2.05 M chromium (III) chloride and 12.5 mL of 2.05 M sodium carbonate. a. What is the limiting reactant? b. What is the theoretical yield in mass of chromium (III) carbonate? c. What is the experimental yield if the percent yield is 62.5%? Chapter 9: Gases 9. Determine the density of the gases at STP: a. Chlorine b. Oxygen difluoride c. Dinitrogen monoxide d. Krypton 10. Determine the density of the gases in number 12 when the temperature is 165ºC and under 1.978 atm of pressure. 11. Determine the volume of the gases: a. 24.5 mol of carbon monoxide under 0.675 atm of pressure at ?40.0ºC. b. 24.5 g of carbon monoxide under 0.675 atm of pressure at ?40.0ºC. c. 88.0 g of argon under 5.09 atm of pressure at 350 ºC. d. 88.0 g of neon under 5.09 atm of pressure at 350 ºC. e. 1.75 mol of nitrogen dioxide under 2.04 atm of pressure at 110 ºC. 12. Determine how the previous volumes will (or will not) change if the gas was changed to hydrogen. 13. Determine the pressure of the gases: a. 24.5 mol of carbon monoxide in a 250 L container at ?40.0ºC. b. 24.5 g of carbon monoxide in a 250 L container at ?40.0ºC. c. 88.0 g of argon in a 40.0 L container at 350 ºC. d. 88.0 g of neon in a 40.0 L container at 350 ºC. e. 1.75 mol of nitrogen dioxide in a 100.0 L container at 110 ºC. 14. Determine how the previous pressures will (or will not) change if the gas was changed to hydrogen. 15. Determine the temperature of the gases: a. 24.5 mol of carbon monoxide in a 250 L container under 2.675 atm of pressure. b. 24.5 g of carbon monoxide in a 250 L container under 0.675 atm of pressure. c. 88.0 g of argon in a 15.0 L container under 5.09 atm of pressure. d. 88.0 g of neon in a 15.0 L container under 5.09 atm of pressure. e. 1.75 mol of nitrogen dioxide in a 25.0 L container under 2.04 atm of pressure. 16. Determine how the previous temperatures will (or will not) change if the gas was changed to hydrogen. 17. Determine the mass of the gas under the conditions. a. 24.5 L of carbon monoxide under 1.675 atm of pressure at 40 °C. b. 24.5 L of nitrogen monoxide under 1.675 atm of pressure at 40°C. c. 40.0 L of krypton under 5.09 atm of pressure at ?25°C. d. 40.0 L of helium under 5.09 atm of pressure at ?25°C. e. 10.0 L of nitrogen dioxide under 2.04 atm of pressure at 125 °C. f. 100.0 L of carbon dioxide under 0.156 atm of pressure at 0°C 18. Determine the molar mass of the gases in a 25.5 L container. a. 125 g of a gas under 1.85 atm of pressure at 95.6 ºC. b. 12.78 g of a gas under 0.756 atm of pressure at 22.2 ºC. c. 4.55 g of a gas under 0.156 atm of pressure at ?57.5 ºC. d. 1.25 g of a gas under 0.325 atm of pressure at ?110. ºC. e. 4.56 g of a gas under 0.1705 atm of pressure at 75.6 ºC. f. 15 g of a gas under 0.506 atm of pressure at 62.4 ºC. 19. Using the balanced chemical reaction, determine the desired quantity: ( ) ( ) ( ) ( )3 2 24 6 5 6NH g NO g N g H O l+ ? + a. The mass of water produced from 12.35 L of ammonia under 0.956 atm of pressure at 105 ºC and excess nitrogen monoxide. b. The mass of water produced from 12.35 L of nitrogen monoxide under .956 atm of pressure at 105 ºC and excess ammonia. c. The volume of nitrogen produced when 42 L of ammonia is consumed under STP. d. The volume of nitrogen produced when 42 L of nitrogen monoxide is consumed under STP. e. The total volume of gases consumed when 55.0 g of water is produced at STP. f. The volume of nitrogen produced under STP when 55.0 g of water is also produced. Anja Blecking Microsoft Word - Final_Exam_worksheet