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Ideal Gas Law & Gas Stoichiometry

PV = nRT. R = 0.0821 L atm/molK = 8.315 dm 3 kPa/molK. Ideal Gas Law & Gas Stoichiometry. 1) Work out each problem on scratch paper. 2) Click ANSWER to check your answer. 3) Click NEXT to go on to the next problem. CLICK TO START. QUESTION #1.

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Ideal Gas Law & Gas Stoichiometry

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  1. PV = nRT R = 0.0821 Latm/molK = 8.315 dm3kPa/molK Ideal Gas Law & Gas Stoichiometry 1) Work out each problem on scratch paper. 2) Click ANSWER to check your answer. 3) Click NEXT to go on to the next problem. CLICK TO START

  2. QUESTION #1 • How many grams of CO2 are produced from 75 L of CO at 35°C and 96.2 kPa? • 2CO + O2 2CO2 ANSWER

  3. ANSWER #1 PV = nRT V = 26.6 dm3/mol • Find the new molar volume: • n = 1 mol • V = ? • P = 96.2 kPa • T = 35°C = 308 K • R = 8.315 dm3kPa/molK BACK TO PROBLEM CONTINUE...

  4. ANSWER #1 (con’t) 2CO + O2 2CO2 75 L ? g 75 L CO 1 mol CO 26.6 L CO 2 mol CO2 2 mol CO 44.01 g CO2 1 mol CO2 = 120 g CO2 BACK TO PROBLEM NEXT

  5. QUESTION #2 • How many moles of oxygen will occupy a volume of 2.5 L at 1.2 atm and 25°C? ANSWER

  6. ANSWER #2 PV = nRT n = 0.12 mol • n = ? • V = 2.5 L • P = 1.2 atm • T = 25°C = 298 K • R = 0.0821 Latm/molK BACK TO PROBLEM NEXT

  7. QUESTION #3 • What volume will 56.0 grams of nitrogen (N2) occupy at 96.0 kPa and 21°C? ANSWER

  8. ANSWER #3 PV = nRT V = 50.9 dm3 • V = ? • n = 56.0 g = 2.00 mol • P = 96.0 kPa • T = 21°C = 294 K • R = 8.315 dm3kPa/molK BACK TO PROBLEM NEXT

  9. QUESTION #4 • What volume of NH3 at STP is produced if 25.0 g of N2 is reacted with excess H2? • N2 + 3H2 2NH3 ANSWER

  10. ANSWER #4 N2 + 3H2 NH3 25.0 g ? L 25.0 g N2 1 mol N2 28.02 g N2 2 mol NH3 1 mol N2 22.4 L NH3 1 mol NH3 = 40.0 L NH3 BACK TO PROBLEM NEXT

  11. QUESTION #5 • What volume of hydrogen is produced from 25.0 g of water at 27°C and 1.16 atm? • 2H2O  2H2 + O2 ANSWER

  12. ANSWER #5 PV = nRT V = 21.2 L/mol • Find the new molar volume: • n = 1 mol • V = ? • P = 1.16 atm • T = 27°C = 300. K • R = 0.0821 Latm/molK BACK TO PROBLEM CONTINUE...

  13. ANSWER #5 (con’t) 2H2O  2H2 + O2 25.0 g ? L 25.0 g H2O 1 mol H2O 18.02 g H2O 2 mol H2 2 mol H2O 21.2 L H2 1 mol H2 = 29.4 L H2 BACK TO PROBLEM NEXT

  14. QUESTION #6 • How many atmospheres of pressure will be exerted by 25 g of CO2 at 25°C and 0.500 L? ANSWER

  15. ANSWER #6 PV = nRT P = 28 atm • P = ? • n = 25 g = 0.57 mol • T = 25°C = 298 K • V = 0.500 L • R = 0.0821 Latm/molK BACK TO PROBLEM NEXT

  16. QUESTION #7 • How many grams of CaCO3 are required to produce 45.0 dm3 of CO2 at 25°C and 2.3 atm? • CaCO3 + 2HCl  CO2 + H2O + CaCl2 ANSWER

  17. ANSWER #7 PV = nRT V = 11 L/mol • Find the new molar volume: • n = 1 mol • V = ? • P = 2.3 atm • T = 25°C = 298 K • R = 0.0821 Latm/molK BACK TO PROBLEM CONTINUE...

  18. ANSWER #7 CaCO3 + 2HCl  CO2 + H2O + CaCl2 ? g 45.0 dm3 45.0dm3 CO2 1 mol CO2 11 dm3 CO2 1 mol CaCO3 1 mol CO2 100.09 g CaCO3 1 mol CaCO3 = 410 g CaCO3 BACK TO PROBLEM NEXT

  19. QUESTION #8 • Find the number of grams of CO2 that exert a pressure of 785 torr at 32.5 L and 32°C. ANSWER

  20. ANSWER #8 PV = nRT n = 1.34 mol  59.0 g CO2 • n = ? • P = 785 torr = 1.03 atm • V = 32.5 L • T = 32°C = 305 K • R = 0.0821 Latm/molK BACK TO PROBLEM NEXT

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