6-The following reaction takes place into a constant-volume flask at 427C: CC14(E) = C(s) + 2 C12(E) AH=132 kJ At 427C, the equilibrium constant for the reaction given above is K = 1.3x10-2 A flask is filled with 2.00 atm of CCL at 427C. (a) What is the value of K, for this reaction? (R=0.082 L. atm mol.K) (6) What are the partial pressures of CCL, Cl, and the total pressure at equilibrium? C) How will the equilibrium pressure of CCL(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced