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# At $500^{\circ} \mathrm{C}$, the reaction$\mathrm{SO}_2(g)+\mathrm{NO}_2(g) \rightleftharpoons \mathrm{NO}(g)+\mathrm{SO}_3(g)$has $K_{\mathrm{oq}}=81$. What will be the equilibrium concentrations of the four gases if the two reactants begin with equal concentrations of $0.50~M$ ?

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In this task, we need to calculate equilibrium concentrations of gases.

For the reaction:

$\text{aA}+\text{bB} \rightleftharpoons \text{cC} +\text{dD}$

the K$_{eq}$ is:

$K_{eq}=\dfrac{[\text{C}]^c[\text{D}]^d}{[\text{B}^b][\text{A}]^a}$

The equilibrium constant is equal to the product of the concentration of the products raised to the potency of its stoichiometric factor divided by the product of the concentration of the reactants raised to the potency of its stoichiometric factor.

Using the $K_{eq}$ we can calculate $x$. When we know the $x$ (change) we can calculate equilibrium concentrations.

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