If a gas is moved from a large container to a small container but its temperature and number of moles remain the same, what would happen to the pressure of the gas?

It would increase

It would be halved

It would stay the same

It would slightly decrease

To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 = P2V2

P2 = P1V1/V2

The correct answer is the first option. Pressure would increase. This can be seen from the equation above where V2 is indirectly proportional to P2.