Which change would increase the pressure exerted by a gas? removing gas molecules from the container transferring the gas to a larger container raising the temperature of the gas reducing the force of the molecules hitting the container

Option (c) is the correct answer.

Explanation:

According to the ideal gas equation, product of pressure and volume of a gas is directly propotional to the temperature.

The equation for ideal gas is as follows.

                  PV = nRT

where,       n = number of moles

                 R = gas constant

Therefore, when we increase the temperature then there will be more collisions between the gas particles. As a result, there will be increse in kinetic energy of molecules thus, there will be increase in pressure on each particle. Hence, increase in temperature would increase the pressure exerted by a gas.

Whereas if we remove gas molecules from the container then there will be no particles at all inside the container. Thus, there will be decrease in pressure as there are no particles available for collision.

From the ideal gas equation, it can be seen that pressure is inversely proportional to volume. When we transfer gas molecules to a larger container then we are providing more space to the gas particles. Thus, there will be decrease in pressure as the volume is increased.

When we reduce force of the molecules hitting the container then there will be less number of collisions between the particles. As a result, there will be decrease in pressure.

Hence, we can conclude that out of the given options, raising the temperature of the gas would increase the pressure exerted by a gas.

i think that the answer is c