Question

For the reversible reaction :
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)+heat$
The equilibrium shifts in forward direction-

• A. By increasing the concentration of $N{H}_3\left(g\right)$
• B. By decreasing the pressure
• C. By decreasing the concentrations of $N_2\left(g\right)$ and $H_2\left(g\right)$
• D. By increasing pressure and decreasing temperature

Answer 1

The correct option is D By increasing pressure and decreasing temperature

The given reaction is exothermic as heat is released during the reaction.
For an exothermic reaction, on decreasing the temperature equilibrium will shift in forward direction.
According to the Le Chatelier's principle, on increasing pressure, equilibrium will shift in the direction where lesser number of gaseous moles are present. Hence, on increasing pressure equilibrium will shift in forward direction for the given system.