- 1(current)
Q. No.\([ Given: \Delta \mathrm{H}\) of the reaction \(=+180.7 \mathrm{~kJ} \mathrm{~mol}^{-1} ]\)
A. higher temperature
B. lower temperature
C. higher concentration of \(\mathrm{N}_2\)
D. higher concentration of \(\mathrm{O}_2\)
Choose the correct answer from the options given below:
1. B, C, D only
2. A, C, D only
3. A, D only
4. B, C only
In light of the above facts, which of the following is correct?
| 1. | Reaction has a tendency to go in the forward direction. |
| 2. | Reaction has a tendency to go in the backward direction. |
| 3. | Reaction has gone to completion in the forward direction. |
| 4. | Reaction is at an equilibrium. |
\(\mathrm{N_2(g) +3H_2(g) \rightleftharpoons 2NH_3(g), \Delta H=-Q}\)
Reaction is favoured in forward direction by:
| 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.
What conditions favor the formation of 2XY₄(g) in the reaction X₂(g) + 4Y₂(g) ⇋ 2XY₄(g), considering that the enthalpy change (ΔH) is negative?
1. Low pressure and low temperature
2. High temperature and low pressure
3. High pressure and low temperature
4. High temperature and high pressure
- 1(current)
Q. No.
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