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?

Explanation:

According to ideal gas law, product of pressure and volume equals the product of number of moles, gas constant and temperature.

Mathematically,     PV = nRT

Therefore, it can be seen that volume is inversely proportional to pressure. So, when gas is moved from a large container to a small container then it means volume of container is reduced.

Hence, pressure on the gas will increase and this will tend to compress the gas.