P*V = n*R*T where P = pressure V = volume n = number of moles R = the universal gas constant T = temperature in degrees Kelvin This equation is known as the ideal gas law, and it can be used to predict the behavior of many gases at relatively low pressure. From this equation, you can see that as the temperature of a gas increases, A) the pressure of the gas increases. B) the number of moles of gas will go down. C) either the pressure of the gas, the volume of the gas, or both, will increase. D) either the pressure of the gas, the volume of the gas, or both, will decrease.

(C) either the pressure of the gas, the volume of the gas, or both, will increase

Explanation:

From the ideal gas law given;

P*V = n*R*T

↓

T ∝ P*V

Temperature of the gas is directly proportional to pressure and volume of the gas.

Therefore, for a given number of moles and increasing temperature; either the pressure of the gas, the volume of the gas, or both, will increase

The Gay-Lussac's law or Amonton's law states that the pressure of a given amount of a gas is directly propotional to its temperature if its volume is kept constant.

P∝T

and

The Charles Law states that volume of given amount of gas at constant pressure is directly propotional to temperature.

V∝T

So, by Gay-Lussac's law if we increase the temperature the Pressure will increase and by Charles Law, if we increase the temperature the volume will increase.

Therefore, if the temperature of gas increases either the pressure of the gas, the volume of the gas, or both, will increase.

Hence,

Answer is option C