For the reaction,

  PCl₅(g) $\rightleftharpoons$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

The following reactions are known to occur in the body,

    CO₂ + H₂O$\rightleftharpoons$H₂CO₃$\rightleftharpoons$H⁺ + HCO₃^-                 

If CO₂ escapes from the system, then:

1. pH will decrease

2. hydrogen ion concentration will diminish

3. H₂CO₃ concentration will be unaltered

4. the forward reaction will be promoted

According to Le-Chatelier's principle, adding heat to a solid $\rightleftharpoons$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

Which oxide of nitrogen is the most stable?

1. 2NO₂(g) $\rightleftharpoons$N₂(g) + 2O₂(g);         K=6.7x10¹⁶ mol litre^-1

2. 2NO(g) $\rightleftharpoons$N₂(g) + O₂(g);            K=2.2x10³⁰ mol litre^-1

3. 2N₂O₅(g) $\rightleftharpoons$2N₂(g) + 5O₂(g);      K=1.2x10³⁴ mol^-5 litre^-5

4. 2N₂O(g) $\rightleftharpoons$2N₂(g) + O₂(g);         K=3.5x10³³ mol litre^-1

For the chemical reaction, $3\mathrm{X}\left(\mathrm{g}\right) + \mathrm{Y}\left(\mathrm{g}\right) \rightleftharpoons {\mathrm{X}}_3\mathrm{Y}\left(\mathrm{g}\right)$;

the amount of X₃Y at equilibrium is affected by :

1. Temperature and pressure

2. Temperature only

3. Pressure only

4. Temperature, pressure and catalyst

Solubility of a gas in liquid increases on:

1. Addition of a catalyst

2. Increasing the pressure

3. Decreasing the pressure

4. Increasing the temperature

The equilibrium, 2SO₂ (g) + O₂ (g) $\rightleftharpoons$2SO₃ (g)

shifts forward if:

1. a catalyst is used

2. an absorbent is used to remove SO₃ as soon as it is formed

3. small amounts of reactants are used

4. none of the above

The value of $∆$H for the reaction,

   X₂(g) + 4Y₂(g) $\rightleftharpoons$2XY₄ (g)

is less than zero. Formulation of XY₄(g) will be favored 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

On addition of inert gas at constant volume to the reaction, N₂ + 3H₂$\rightleftharpoons$2NH₃ at  equilibrium:

1. the reaction halts

2. forward reaction is favored

3. the reaction remains unaffected

4. backward reaction is favored

For the reversible reaction,

N₂ (g) + 3H₂(g) $\rightleftharpoons$2NH₃ (g) + heat

 the equilibrium shifts in forward direction                                   

1. by increasing the concentration of NH₃ (g) 

2. by decreasing the pressure

3. by decreasing the concentrations of N₂ (g)and H₂(g)

4. by increasing pressure and decreassing temperature