Consider the following equilibrium for which H = -108.6 kJ:
CO(g) + Cl2(g) COCl2(g)
If a mixture of the gases involved in this reaction is allowed to
come to equilibrium, and
some COCl2 is removed from this
equilibrium mixture, decreasing the partial pressure
of COCl2, what will the reaction do in response to
this change, and how will the value of K (the equilibrium constant)
be affected?
a) The reaction will shift toward products with no change in
K.
b) The reaction will not shift and the value of K will not
change.
c) The reaction will shift toward reactants with an increase in
K.
d) The reaction will shift toward reactants with no change in
K.
e) The reaction will shift toward products with a decrease in
K.