Which of these changes would not cause an increase in the pressure of a contained gas a. the volume of the container is increased b. more of the gas is added to the container c. the temperature is increased d. the average kinetic energy of the gas increased

Option (a) is the correct answer.

Explanation:

According to the ideal gas equation, PV = nRT.

Hence, pressure is inversely proportional to volume. So, when volume of container is increased then there will be decrease in pressure and vice-versa.

As pressure is directly proportional to number of moles. So, when there is more number of moles of gas then there will also be increase in pressure.

Also, temperature is proportional to pressure. So, an increase in temperature will lead to increase in pressure.

Average kinetic energy of molecules of gas will increase due to increase in temperature. Hence, this will lead to increase in pressure also.

Thus, we can conclude that out of the given options when the volume of the container is increased then it would NOT cause an increase in the pressure of a contained gas.

c. 75.7

i think that is the right

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