A gas sample containing 0.3250 moles of a compound is trapped in a chamber with a volume of 2.460 liters. If the temperature of the gas is 26.8 °C, what is its pressure? Assume the gas exhibits ideal gas behavior.

Question

Quizplus · Accepted Answer

To find the pressure, use the ideal gas law: PV = nRT. Convert the temperature to Kelvin (26.8 + 273.15 = 299.95 K). Use R = 0.0821 L·atm/mol·K. Solve for P: P = (nRT)/V = (0.3250 mol × 0.0821 L·atm/mol·K × 299.95 K) / 2.460 L = 3.252 atm. Convert atm to torr (1 atm = 760 torr): 3.252 atm × 760 torr/atm = 2471.52 torr, which rounds to 2471 torr.

A Gas Sample Containing 0