At 700 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.2 atm at equilibrium. P=?

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

Therefore, the law of mass action is:

Pressure of carbon at equilibrium is not considered since it is solid. In such a way, based on the law of mass action, at equilibrium we have:

And in the law of mass action:

Now, from the total pressure, we have that:

And we combine:

Thus, solving for we have to roots:

Clearly, the solution must be 0.323 atm, in such a way, the initial pressure turns out:

Regards.

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: