At 700 K the equilibrium constant for the reaction
CCl4(g) <===> C(s) + 2 Cl2(g)
is Kp = 0.76. A flask is charged with 2.00 atm CCl4, which then reaches equilibrium at 700 K.
(a) What fraction of the CCl4 is converted into C and Cl2;
(b) What are the partial pressures of CCl4 and Cl2 at equilibrium?