WAEC - Chemistry (2018 - No. 12)
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 decrease in pressure
an increase in pressure
a decrease in temperature
an introduction of a positive catalyst
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).
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