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  • Need clarity, kindly explain! - Equilibrium - JEE Main-2

The exothermic formation of ClF_{3} is represented by the equation:

Cl_{2(g)}+3F_{2(g)}\rightleftharpoons 2ClF_{3(g)};\Delta H= -329 kJ

Which of the following will increase the quantity of ClF_{3}     in an equilibrium mixture of Cl_{2},F_{2},and ClF_{3}

  • Option 1)

    increasing the temperature

  • Option 2)

    Removing  Cl_{2}

  • Option 3)

    increasing the volume of the container

  • Option 4)

    Adding F_{2}

 

Answers (1)

As we learnt in 

Effect of concentration change on equilibrium -

When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium mixture changes so as to minimize the effect of concentration change. If we add reactant, the equilibrium shift towards right.

-

 

 

Cl_{2(g)}+3F_{2(g)}\rightleftharpoons 2ClF_{3(g)};\Delta H= -329 kJ

Favourable conditions:

(i) As the reaction is exothermic, hence decrease in temperature will favour the forward reaction.

(ii) Addition of Cl2 or F2 or both and removal of ClF3 favour the forward reaction.

(iii) Here \Delta n = 2 - 4 = -2 (i.e. , -ve) hence decrease in volume or increase in pressure will favour the forward reaction..


Option 1)

increasing the temperature

This option is incorrect

Option 2)

Removing  Cl_{2}

This option is incorrect

Option 3)

increasing the volume of the container

This option is incorrect

Option 4)

Adding F_{2}

This option is correct

Posted by

Sabhrant Ambastha

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