Consider the following equilibrium reaction: (2AB_{{2}{(g)}} + B_{{2}{(g)}} to 2AB_{{3}{(g)}}). (Delta H= -X kJmol^{-1}). The backward reaction will be favored by
-
A.
a decrease in pressure -
B.
an increase in pressure -
C.
a decrease in temperature -
D.
an introduction of a positive catalyst
Correct Answer: Option A
Explanation
The equilibrium position is shifted to the left with a decrease in pressure in this system because the number of gaseous molecules on the right is less. (Le-Chatelier’s principle).