Question #63428
Chapter 15 (15.87)

At 700 K the equilibrium constant for the reaction
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K.

1) What fraction of the CCl4 is converted into C and Cl2?

2) What is the partial pressure of CCl4 at equilibrium?

3) What is the partial pressure of Cl2 at equilibrium?
1
Expert's answer
2016-11-20T18:53:13-0500
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