The exothermic formation of $\mathrm{ClF}_{3}$ is represented by the equation:…

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

Solution

The reaction given is an exothermic reaction thus according to Le chatalier's principle lowering of temperature, addition of $\mathrm{F}_{2}$ and $\mathrm{Cl}_{2}$ favour the forward direction and hence the production of $\mathrm{ClF}_{3}$. ,

Asked in: JEE-TOPICTESTS-CHEMISTRY

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