JEE Main 2005

Question

The exothermic formation of $	ext{ClF}_3$ is represented by the equation:
$	ext{Cl}_2(g) + 3	ext{F}_2(g) ightleftharpoons 2	ext{ClF}_3(g);\ \Delta H = -329	ext{ kJ}$
Which of the following will increase the quantity of $	ext{ClF}_3$ in an equilibrium mixture of $	ext{Cl}_2$, $	ext{F}_2$ and $	ext{ClF}_3$? A). Adding $	ext{F}_2$ B). Increasing the volume of the container C). Removing $	ext{Cl}_2$ D). Increasing the temperature

Edvaya · Accepted Answer

The correct answer is Adding $	ext{F}_2$. By Le Chatelier's principle:
- Adding a reactant ($	ext{F}_2$) shifts the equilibrium to the right, producing more $	ext{ClF}_3$.
- Increasing volume decreases pressure, shifting equilibrium to the side with more moles (left).
- Removing $	ext{Cl}_2$ shifts the equilibrium to the left.
- Increasing temperature for an exothermic reaction shifts the equilibrium to the left.
Thus, only adding $	ext{F}_2$ increases the quantity of $	ext{ClF}_3$.

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Chemistry > Physical Chemistry > Equilibrium

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