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NEET CHEMISTRYMedium

For the reversible reaction: N2(g)+3H2(g)⇌2NH3(g)+heatN_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat}. The equilibrium shifts in a forward direction:

A

by increasing the concentration of NH3(g)NH_3(g)

B

by decreasing the pressure.

C

by decreasing the concentration of N2(g)N_2(g) and H2(g)H_2(g)

D

by increasing pressure and decreasing temperature.

Step-by-Step Solution

According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the equilibrium shifts in a direction that tends to undo the effect of the change.

  1. Temperature: The forward reaction is exothermic (releases heat). Therefore, decreasing the temperature will favour the forward reaction to produce more heat.
  2. Pressure: The forward reaction proceeds with a decrease in the number of moles of gas (from 4 moles of reactants to 2 moles of product). Therefore, an increase in pressure will shift the equilibrium in the direction that has fewer moles of gas, which is the forward direction. Thus, high pressure and low temperature favour the forward reaction.
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