Two one-liter containers each contain 10 moles of a gas.The temperature is the same in both containers.Container A holds helium (molecular mass = 4 u),and Container B holds oxygen (molecular mass = 16 u).Which container has the higher pressure and by what factor?
A)Container A has 4 times the pressure of Container B.
B)Container A has 2 times the pressure of Container B.
C)Both containers have the same pressure.
D)More information is needed to answer this question.

Question

Quizplus · Accepted Answer

The pressure of a gas in a container (assuming ideal gas behavior) is determined by the equation PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature. Since both containers have the same volume, number of moles, and temperature, and since the ideal gas law does not depend on the type of gas, both containers have the same pressure.

Two One-Liter Containers Each Contain 10 Moles of a Gas