WAEC - Chemistry (2013 - No. 33)
Consider the reaction represented by the equation: N\(_2\)O\(_4\)(g) ⇌ 2NO\(_2\)(g) ; ∆H = + x kJmol-1
What happens when the temperature is reduced at equilibrium?
What happens when the temperature is reduced at equilibrium?
Concentration of N 2O4(g) decreases
Concentration of N 2O4(g) increases.
Pressure exerted by the gases increases
Pressure exerted by the gases remains constant
Explanation
According to Le Chatelier's principle, in an endothermic reaction(ΔH = +ve), an increase in temperature will cause the equilibrium to shift to the right, thereby favouring the forward reaction, and more product will be formed. Conversely, in an endothermic reaction, a decrease in temperature will cause the equilibrium position to shift to the left, thereby favouring the backward reaction, and more reactants(N\(_2\)O\(_4\)) will be produced.i.e Concentration of N\(_2\)O\(_4\) will increase.
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