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?

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?

A) 334.6 torr B) 2513 torr C) 2694 torr D) 2510 torr E) 2007 torr

Solution: We are given the number of moles, volume, and temperature. We can use the Idea Gas Law to find pressure.

PV=nRT where P is pressure in atm, V is volume in L, n is the number of moles, R is the ideal gas constant and T is temperature in Kelvin.

P = ?

V = 2.641 L

n = 0.3525 moles

R = 0.08206 L*atm/mol*K

T = 28.4 °C +273 = 301.4K

P(2.641 L)=0.3525 moles* 0.08206 L*atm/mol*K*301.4K

P = 3.30atm (760torr/1atm) = 2510 torr, choice D

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