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Introduction to Le Chatelier's Principle

The exothermi...

Question

The exothermic formation of $C l F_{3}$ is represented by the equation $C l_{2 (g)} + 3 F_{2 (g)} ⇌ 2 C l F_{3 (g)}$ ; $Δ H = - 329 k J$ . Which of the following will increase the quantity of $C l F_{3}$ in an equilibrium mixture of $C l_{2}, F_{2}$ and $C l F_{3} ?$

A

Increasing the temperature

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B

Removing

C l_{2}

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C

Increasing the volume of the container

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D

Adding

F_{2}

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Solution

The correct option is D Adding $F_{2}$
The formation of $C l F_{3}$ is represented by the equation $C l_{2 (g)} + 3 F_{2 (g)} ⇌ 2 C l F_{3 (g)}$ ; $Δ H = - 329 k J$ .
According to the Le-chatelier`s principle if any changes happen in any component then equilibirium will move that direction where the effect of that change neutralize.

(a)As this reaction is exothermic so on increasing the tempreture the reaction will go in backward direction hence this is not suitable for $C l F_{3}$ to increase.

(b)On removing $C l_{2}$ reaction will go in backward direction hence this is not suitable for $C l F_{3}$ to increase.

(c)On increasing the volume the reaction would go towards more no. of moles which means reaction will go in backward direction hence this is not suitable for $C l F_{3}$ to increase.

(d)On adding $F_{2}$ reaction will go in forward direction hence this is suitable for $C l F_{3}$ to increase.

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Similar questions

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Introduction to Le Chatelier's Principle

Standard XII Chemistry

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