For the reversible reaction,
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g) + heat
The equilibrium shifts in forward direction
A
by increasing the concentration of NH3(g)
B
by decreasing the pressure
C
by decreasing the concentrations of N2(g) and H2(g)
D
by increasing pressure and decreasiing temperature.
Explanation
According to Le-Chatelier’s principle, the
equilibrium shifts in that direction so as to oppose
the applied change.
Given reaction is exothermic reaction. Hence
according to Le-Chatelier's principle low
temperature favours the forward reaction and
on increasing pressure equilibrium will shift,
towards lesser number of moles i.e. forward
direction.
2
AIPMT 2014
MCQ (Single Correct Answer)
For a given exothermic reaction, Kp and K'p are the equilibrium constants at temperatures T1 and T2, respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is readily observed that