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5. Consider the decomposition of the compound $\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}$ as follows:
$\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g})+3 \mathrm{CO}(\mathrm{g})$
When a 5.63-g sample of pure $\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}(\mathrm{~g})$ was sealed into an otherwise empty 2.50-L flask and heated to $200 .{ }^{\circ} \mathrm{C}$, the pressure in the flask gradually rose to $1.63 \mathrm{~atm}$ and remained at that value. Calculate $\mathrm{K}$ for this reaction.
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Answer from Sia

Posted 5 months ago

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Answer

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Key Concept

The equilibrium constant $K_p$ is calculated using the partial pressures of the reactants and products at equilibrium.

Explanation

To find $K_p$, we need to determine the moles of reactants and products at equilibrium, convert those to partial pressures, and then apply the equilibrium expression.

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