For the following reaction,
H
The effect on the state of equilibrium on doubling the volume of the system will be:
1. | Shift to the reactant side | 2. | Shift to the product side |
3. | No effect on the state of equilibrium | 4. | Liquefaction of HI |
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.
Given a hypothetical reaction :
More could be produced at equilibrium by :
1. | Using a catalyst | 2. | Removing some of B2 gas |
3. | Increasing the temperature | 4. | Increasing the pressure |
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
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. |
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)
1. Only (iii)
2. Only (ii)
3. Both (i) and (ii)
4. None of the above.
(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
For the reaction,
PCl5(g) PCl3(g) + Cl2 (g)
The forward reaction at constant temperature is favoured by:
1. Introducing an inert gas at a constant volume
2. Introducing chlorine gas at a constant volume
3. Introducing an inert gas at constant pressure
4. None of the above
Inert gas is added to the equilibrium at constant pressure. The degree of dissociation will :
1. Remain unchanged
2. Decrease
3. Increase
4. Decrease or increase but cannot be predicted with certainty
According to Le-Chatelier's principle, adding heat to a solid liquid equilibrium will cause the :
1. Temperature to increase
2. Temperature to decrease
3. Amount of liquid to decrease
4. Amount of solid to decrease