Ideal Gas Law 1 (Equation: PV=nRT) - Check

Known: n = 0.248 mol P = 900.0 mmHg x 1 atm / 760 mmHg = 1.184 atm V = 750.0 mL x 1 L / 1000 mL = 0.7500 L R = 0.0821 L atm/mol K

Question: At what temperature will 0.248 moles of neon (Ne) gas exert a pressure of 900.0 mmHg at a volume of 750.0 mL? (1) Identify all the KNOWN amounts given in the problem.

Unknown: T = PV / nR = 1.184 atm x 0.7500 L / 0.248 mol x 0.0821 L atm/mol K Final Answer: 43.6 K #SF: 3

Question: At what temperature will 0.248 moles of neon (Ne) gas exert a pressure of 900.0 mmHg at a volume of 750.0 mL? (2) Calculate the UKNOWN. Identify the number of significant figures (#SF) in the final answer.

Known: V = 350 mL x 1 L / 1000 mL = 0.35 L P = 6660 torr x 1 atm / 760 torr = 8.76 atm T = 29 C + 273 = 302 K R = 0.0821 L atm/mol K

Question: How many moles of ammonia gas (NH3) will occupy a volume of 350 mL at 6660 torr and 27 C? (1) Identify all the KNOWN amounts given in the problem.

Unknown: n = PV / RT = 8.76 atm x 0.35 L / 0.0821 L atm / mol K x 302 K Final Answer: 0.12 mol #SF: 2

Question: How many moles of ammonia gas (NH3) will occupy a volume of 350 mL at 6660 torr and 27 C? (2) Calculate the UKNOWN. Identify the number of significant figures (#SF) in the final answer.

Known: V = 2.5 L P = 1.2 atm T = 25 C + 273 = 298 K R = 0.0821 L atm/mol K

Question: How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25 C. (1) Identify all the KNOWN amounts given in the problem.

Unknown: n = PV / RT = 1.2 atm x 2.5 L / 0.0821 L atm/mol K x 298 K Final Answer: 0.12 mol #SF = 2

Question: How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25 C. (2) Calculate the UKNOWN. Identify the number of significant figures (#SF) in the final answer.

Known: n = 0.893 mol T = 25 K + 273 = 298 K V = 500.0 mL x 1L / 1000 mL = 0.5000 L R = 0.0821 L atm/mol K

Question: What pressure will be exerted by 0.893 moles of carbon monoxide (CO) gas at a temperature of 25 C and a volume of 500.0 mL? (1) Identify all the KNOWN amounts given in the problem.

Unknown: P = nRT / V = 0.893 mol x 0.0821 L atm/mol K x 298 K / 0.5000 L Final Answer: 43.7 atm #SF: 3

Question: What pressure will be exerted by 0.893 moles of carbon monoxide (CO) gas at a temperature of 25 C and a volume of 500.0 mL? (2) Calculate the UKNOWN. Identify the number of significant figures (#SF) in the final answer.

Known: n = 2.0 mol P = 720 torr x 1 atm / 760 torr = 0.95 atm T = 20 C = 273 = 293 K R = 0.0821 L atm/mol K

Question: What volume will 2.0 moles of nitrogen occupy at 720 torr and 20 C? (1) Identify all the KNOWN amounts given in the problem.

Unknown: V = nRT / P = 2.0 mol x 0.0821 L atm / mol k x 293 K / 0.95 atm Final Answer: 51 L #SF: 2

Question: What volume will 2.0 moles of nitrogen occupy at 720 torr and 20 C? (2) Calculate the UKNOWN. Identify the number of significant figures (#SF) in the final answer.