You fill a tank with gas at 60 C to 100 kpa and seal it you decrease the temperature to 10

The given question is incomplete. The complete question is :

You fill a tank with gas at 60C and 100 kPa and seal it. You decrease the temperature to 10C but keep the volume constant. What happens to the pressure?

Thus the pressure will decrease to 85.0 kPa

Explanation:

Gay-Lussac's Law : It is defined as the pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

(Volume, moles of gas are constant)

Mathematically,

where,

are the initial pressure and temperature of the gas.

are the final pressure and temperature of the gas.

We are given:

Putting values in above equation, we get:

Thus the pressure will decrease to 85.0 kPa

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: