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Question

# Write the equilibrium constant expressions for these reactions:(a) $3 \mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{O}_3(g)$ (b) $\mathrm{H}_2 \mathrm{O}(g) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(l)$ (c) $\mathrm{MgCO}_3(s) \rightleftharpoons \mathrm{MgO}(s)+\mathrm{CO}_2(g)$ (d) $2 \mathrm{~Bi}^{3+}(a q)+3 \mathrm{~H}_2 \mathrm{~S}(a q) \rightleftharpoons \mathrm{Bi}_2 \mathrm{S}_3(s)+6 \mathrm{~H}^{+}(a q)$

Solution

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In this task we need to write equilibrium constant expressions.

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.

For the reaction:

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

the K$_{eq}$ is:

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

Only gaseous and aqueous compounds are included in equilibrium constant expression.

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