At 700 K the equilibrium constant for the reaction CCl4(g) C(s) + 2 Cl2(g) is Kp = 0. A flask is charged with 2.00 atm CCl4, which then reaches…

At 700 K the equilibrium constant for the reactionCCl4(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?