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    Chemical Equilibrium Constant

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    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?

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    Solution Summary

    This solution helps go through problems with regards to chemical equilibrium constant.