Given a cylinder of fixed volume filled with 1 mol of argon gas,which of the following is correct? (Assume all gases obey the ideal gas law. )
A)If the temperature of the cylinder is changed from 25°C to 50°C,the pressure inside the cylinder will double.
B)If a second mole of argon is added to the cylinder,the ratio T/P would remain constant.
C)A cylinder of identical volume filled with the same pressure of helium must contain more atoms of gas because He has a smaller atomic radius than argon.
D)Two of the above.
E)None of the above.

Question

Quizplus · Accepted Answer

A) According to the ideal gas law (PV=nRT), if the temperature of a gas is increased, the pressure will also increase, but not necessarily double unless the temperature is doubled on the Kelvin scale. B) Adding a second mole of argon would increase the pressure if the volume and temperature remain constant, altering the T/P ratio. C) The ideal gas law does not depend on the type of gas or atomic radius but on the amount (moles), volume, temperature, and pressure. Therefore, a cylinder with the same volume and pressure of helium would contain the same number of moles of gas, not necessarily more atoms, since the law considers moles, not atomic or molecular sizes.

Given a Cylinder of Fixed Volume Filled with 1 Mol