What is T2, if T1= 500 k, v1=10L, V2=8L, P1=600 torr, P2=200 torr?

T2 = 133.333°K

Explanation:

Using Combined Gas Laws:

(600 torr)(10L)/500°K = (200 torr)(8L)/x°K

Cross multiply:

x°K (600 torr)(10L) = 500°K(200 torr)(8L)

Divide:

x°K = (500°K(200 torr)(8L))/(600 torr)(10L)

x = 400/3°K or 133.333°K

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: