use the information provided to determine δh°rxn for the following reaction: ch4(g) 4 cl2(g) → ccl4(g) 4 hcl(g) δh°rxn = ?

The given question is incomplete.. The complete question is :

Consider the following reaction:

At equilibrium, a 4.50 L container has 2.6 g of carbon, CO2 at a partial pressure of 0.0020 atm, and a total pressure of 0.572 atm. Calculate KP for this reaction at 725oC.

162.45

Explanation:

Equilibrium pressure of = 0.0020 atm

Total pressure at equilibrium = 0.572 atm

Equilibrium pressure of = Total pressure at equilibrium - Equilibrium pressure of =  (0.572- 0.0020) = 0.570 atm

The given balanced equilibrium reaction is,

At eqm               0        0.0020        0.570

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving we get :

Thus for this reaction at is 162.45