Ideal Gas Law & Gas Stoichiometry

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Presentation transcript:

Ideal Gas Law & Gas Stoichiometry 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

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

V = 26.6 dm3/mol ANSWER #1 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 PV = nRT V = 26.6 dm3/mol BACK TO PROBLEM CONTINUE...

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

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

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

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

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

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

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

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

V = 21.2 L/mol ANSWER #5 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 PV = nRT V = 21.2 L/mol BACK TO PROBLEM CONTINUE...

H2 ANSWER #5 (con’t) 2H2O  2H2 + O2 25.0 g H2O 1 mol H2O 18.02 g BACK TO PROBLEM NEXT

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

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

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

V = 11 L/mol ANSWER #7 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 PV = nRT V = 11 L/mol BACK TO PROBLEM CONTINUE...

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

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

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