For the reaction in equilibrium $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2…
For the reaction in equilibrium
$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-\mathrm{Q}$
Reaction is favoured in forward direction by:
use of catalyst
decreasing concentration of $\mathrm{N}_2$
low pressure, high temperature and high concentration of ammonia
high pressure, low temperature and higher concentration of $\mathrm{H}_2$
Solution
$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-\mathrm{Q}$
According to Le Chatelier's principle.
- Exothermic reactions are favoured at low temperature.
- Increase in pressure shifts the reaction in direction having lesser number of moles. Hence, the given reaction shifts forward on increasing pressure.
- Increasing the concentration of reactants shifts the reaction in forward direction. So high concentration of $\mathrm{H}_2$ shifts reaction in forward direction.