1. | Use of catalyst |
2. | Decreasing concentration of \(\mathrm{N_2}\) |
3. | Low pressure, high temperature and high concentration of ammonia |
4. | High pressure, low temperature and higher concentration of \(\mathrm{H_2}\) |
Mark the conditions that favour the maximum product formation in the given reaction.
1. Low temperature and High pressure
2. Low temperature and Low pressure
3. High temperature and High pressure
4. High temperature and Low pressure
For the reversible reaction:
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g) + heat
The equilibrium shifts in a forward direction:
1. by increasing the concentration of
2. by decreasing the pressure.
3. by decreasing the concentration of
4. by increasing pressure and decreasing temperature.
The value of for the reaction is less than zero. Formation of will be favoured at:
1. Low pressure and low temperature
2. High temperature and low pressure
3. High pressure and low temperature
4. High temperature and high pressure