A gas sample containing 0.3525 moles of a compound is trapped in a 2.641 liter vessel at a temperature of 28.4 °C. What is the pressure in the vessel if the gas behaves as an ideal gas?

Question

Quizplus · Accepted Answer

To find the pressure, use the ideal gas law: PV = nRT. Convert temperature to Kelvin (28.4 + 273.15 = 301.55 K). Use R = 0.0821 L·atm/mol·K. Calculate P = (nRT)/V = (0.3525 mol * 0.0821 L·atm/mol·K * 301.55 K) / 2.641 L = 3.302 atm. Convert atm to torr (1 atm = 760 torr): 3.302 atm * 760 torr/atm = 2510 torr.

A Gas Sample Containing 0