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Q. No.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. |
CH4 (g) + H2O(g) \(\rightleftharpoons\) CO(g) + 3 H2 (g)
then which one of the following changes would cause the equilibrium to shift to the right?
1. Adding Ne(g).
2. Removing some H2O(g).
3. Increasing the pressure.
4. Increasing the temperature.
| 1. | H2(g)+I2(g)⇌2HI(g) |
| 2. | PCl5(g)⇌ PCl3(g)+Cl2(g) |
| 3. | N2(g)+3H2(g)⇌2NH3(g) |
| 4. | The equilibrium will remain unaffected in all the three cases. |
On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,
Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?
| 1. | K will remain the same. |
| 2. | K will decrease. |
| 3. | K will increase. |
| 4. | K will increase initially and then decrease, when pressure is very high. |
\(\mathrm{N_2(g) +3H_2(g) \rightleftharpoons 2NH_3(g), \Delta H=-Q}\)
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 \(\mathrm{H_2}\) |
Sorry!! currently, the explanation for the question is not provided. If you need further help, please email at support@neetprep.com with subject: Explanation Missing for Question Id: 468847
Sorry!! currently, the explanation for the question is not provided. If you need further help, please email at support@neetprep.com with subject: Explanation Missing for Question Id: 468847
When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture it becomes pink
\([Co(H_2O)_6]^{3+} (aq) + 4Cl^-(aq) \rightleftharpoons [CoCl_4]^{2-} (aq) + 6H_2O(l)\\ ~~~\small{(Pink})~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~\small{ (Blue)}\)
On the basis of the information given above, mark the correct answer:
| 1. | ∆ H > 0 for the reaction |
| 2. | ∆ H < 0 for the reaction |
| 3. | ∆ H = 0 for the reaction |
| 4. | The sign of ∆ H cannot be predicted on the basis of the given information. |
(a) PCl5 (g) PCl3 (g) + Cl2 (g)
(b) CaO (s) + CO2 (g) CaCO3 (s)
(c) 3Fe (s) + 4H2O (g) Fe3O4 (s) + 4H2 (g)
The effect of an increase in the volume on the number of moles of products in the above-mentioned reactions would be, respectively:
1. a) Increase, b) decrease, c) same
2. a) Decrease, b) same, c) increase
3. a) Increase, b) increase, c) same
4. a) Increase, b) decrease, c) increase
Consider the following reactions:
(i) COCl2 (g) CO (g) + Cl2 (g)
(ii) CO2 (g) + C (s) 2CO (g)
(iii) 2H2 (g) + CO (g) CH3OH (g)
Which reaction(s) will shift in a backward direction when the pressure is increased?
1. Only (iii)
2. Only (ii)
3. Both (i) and (ii)
4. None of the above.
Given an endothermic reaction:
CH4 (g) + H2O (g) CO (g) + 3H2 (g)
If the temperature is increased, then:
1. The equilibrium will not be disturbed.
2. The equilibrium will shift in the backward direction.
3. The equilibrium will shift in the forward direction.
4. None of the above.
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Q. No.
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