At 700 K the equilibrium constant for the reaction is
CCl4 (g) <--> C (s) + 2 Cl2 (g)
is Kp = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K.
a) What fraction of CCl4 is converted into C and Cl2?
b) What are the partial pressures of CCl4 and Cl2 at equilibrium?© BrainMass Inc. brainmass.com October 10, 2019, 12:10 am ad1c9bdddf
This solution helps go through problems with regards to chemical equilibrium constant.