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For the reversible reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ + heat. The equilibrium shifts in forward direction:
A
by increasing the concentration of $NH_3(g)$
B
by decreasing the pressure
C
by decreasing the concentrations of $N_2(g)$ and $H_2(g)$
D
by increasing pressure and decreasing temperature
Detailed Solution
According to Le Chatelier's principle:
In exothermic reactions, low temperature favours the forward reaction.
On increasing pressure, the equilibrium shifts towards the side with fewer moles of gas.
So the forward reaction is favoured by increasing pressure and decreasing temperature.
In exothermic reactions, low temperature favours the forward reaction.
On increasing pressure, the equilibrium shifts towards the side with fewer moles of gas.
So the forward reaction is favoured by increasing pressure and decreasing temperature.