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 of 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?
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