Q30 / 120 · VITEEE 2007 · Chemistry

For the reaction $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})$, the equilibrium constant $\mathrm{Kp}$ changes with

  • A
    total pressure
  • B
    catalyst
  • C
    the amount $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
  • Correct answer
    D
    temperature

Solution

The equilibrium constant $\mathrm{K}_{\mathrm{p}}$ will change with temperature for the reaction $\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{(\mathrm{g})}$ Catalyst does not alter the state of equilibrium. Equilibrium constant depends only upon temperature. The relation of $k$ with temp can be shown as $\log \frac{k_{2}}{k_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left[\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right]$

Hence, the correct answer is option: 'D'.

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