?At 700 K, the equilibrium constant for the reaction\(\mathrm{CCl}_{4}(g)

Chapter 15, Problem 15.89

(choose chapter or problem)

At 700 K, the equilibrium constant for the reaction

\(\mathrm{CCl}_{4}(g) \rightleftharpoons \mathrm{C}(s)+2 \mathrm{Cl}_{2}(g)\)

is \(K_{p}=0.76\). A flask is charged with 2.00 atm of \(\mathrm{CCl}_{4}\), which then reaches equilibrium at 700 K.

(a) What fraction of the \(\mathrm{CCl}_{4}\) is converted into C and \(\mathrm{Cl}_{2}\) ?

(b) What are the partial pressures of \(\mathrm{CCl}_{4}\) and \(\mathrm{Cl}_{2}\) at equilibrium?

Text Transcription:

CCl_4(g) \rightleftharpoons C(s)+2 Cl_2(g)

K_p=0.76

CCl_4

Cl_2