For the reaction- Cl 2 g -3 F 2 g - 2 ClF 3 g - - H -329 kJ- dissociation of ClF 3 g will be favoured by-A- Decreasing the volume of the containerB- Increasing the temperatureC- Addition of F 2 gasD- Addition of inert gas at constant pressure

The correct option is B Increasing the temperatureFor the reaction, Cl_2(g) nbsp; + 3F_2 (g) ⇌ 2ClF_3(g) ; Δ H = 329 kJ, the dissociation of ClF_3 occur w ...

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Standard XII

Chemistry

Le Chatelier's Principle for Del N Greater Than Zero

For the react...

Question

For the reaction: $C l_{2} (g) + 3 F_{2} (g) ⇌ 2 C l F_{3} (g); Δ H = - 329 kJ$ , dissociation of $C l F_{3} (g)$ will be favoured by:

Increasing the temperature

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Decreasing the volume of the container

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Addition of

F_{2}

gas

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Addition of inert gas at constant pressure

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Solution

The correct option is A Increasing the temperature
For the reaction,
$C l_{2} (g) + 3 F_{2} (g) ⇌ 2 C l F_{3} (g); Δ H = - 329 kJ$ , the dissociation of $C l F_{3}$ occur when the equilibrium shifts towards left.
As it is an exothermic reaction, then increasing the temperature will the equilibrium shifts towards left.

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Similar questions

Q. For the reaction :

{C l}_{2} (g) + 3 F_{2} (g) ⇌ 2 {C l F}_{3} (g);

Δ H = - 329 k J

, dissociation of

{C l F}_{3} (g)

will be favoured by :

For the reaction $P C l_{5} (g) ⇋ P C l_{3} (g) + C l_{2} (g)$ ; the forward reaction at constant temperature is favoured by:

Q. For the reaction:

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

, the forward reaction is favoured by:

Q. Assertion :Addition of inert gases at equilibrium at constant pressure will support the dissociation of

P {C l}_{5}

at a constant temperature. Reason: The addition of inert gas at constant volume will not affect the equilibrium.

Q. For the reaction

P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}

; the forward reaction at constant temperature is favoured by

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For the reaction: Cl2(g)+3F2(g)⇌2ClF3(g); ΔH=−329 kJ, dissociation of ClF3(g) will be favoured by:

The correct option is A Increasing the temperatureFor the reaction, Cl2(g)+3F2(g)⇌2ClF3(g); ΔH=−329 kJ, the dissociation of ClF3 occur when the equilibrium shifts towards left. As it is an exothermic reaction, then increasing the temperature will the equilibrium shifts towards left.

For the reaction: $C l_{2} (g) + 3 F_{2} (g) ⇌ 2 C l F_{3} (g); Δ H = - 329 kJ$ , dissociation of $C l F_{3} (g)$ will be favoured by: