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A vessel of one litre capacity containing 1 mole of $\mathrm{SO}_3$ is heated till a state of equilibrium is attained.
$2 \mathrm{SO}_{3(g)} \rightleftharpoons 2 \mathrm{SO}_{2(g)}+\mathrm{O}_{2(g)}$
At equilibrium, 0.6 moles of $\mathrm{SO}_2$ had formed. The value of equilibrium constant is
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$2 \mathrm{SO}_{3(g)} \rightleftharpoons 2 \mathrm{SO}_{2(g)}+\mathrm{O}_{2(g)}$
At equilibrium, 0.6 moles of $\mathrm{SO}_2$ had formed. The value of equilibrium constant is
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The correct answer is:
$0.68$
$2 \mathrm{SO}_{3(g)} \rightleftharpoons 2 \mathrm{SO}_{2(g)}+\mathrm{O}_{2(g)}$
$\begin{array}{lcl}\text { Inital conc. } 1.0 \text { mole } & 0.0 \text { mole } & 0.0 \text { mole } \\ \text { Equilibrium } 0.4 \text { mole } & 0.6 \text { mole } & 0.3 \text { mole } \\ \Rightarrow \text { Equilibrium constant is given by } \\ K=\frac{\left[\mathrm{SO}_2\right]^2\left[\mathrm{O}_2\right]}{\left[\mathrm{SO}_3\right]^2}=\frac{(0.6)^2(0.3)}{(0.4)^2}=0.675 \approx 0.68\end{array}$
$\begin{array}{lcl}\text { Inital conc. } 1.0 \text { mole } & 0.0 \text { mole } & 0.0 \text { mole } \\ \text { Equilibrium } 0.4 \text { mole } & 0.6 \text { mole } & 0.3 \text { mole } \\ \Rightarrow \text { Equilibrium constant is given by } \\ K=\frac{\left[\mathrm{SO}_2\right]^2\left[\mathrm{O}_2\right]}{\left[\mathrm{SO}_3\right]^2}=\frac{(0.6)^2(0.3)}{(0.4)^2}=0.675 \approx 0.68\end{array}$
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