Question

Write the expression for the equilibrium constant Kc of the following reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) HC3H7CO2 + NH3 equilibrium reaction arrow C3H7CO2− + HNH3+

Answer 1

Answer:

$Kc=\frac{[C_{3}H_{7}CO_{2}^{-} ].[HNH_{3}^{+}]}{[HC_{3}H_{7}CO_{2}].[NH_{3}]}$

Explanation:

The equilibrium constant is calculated as the product of the products raised to the power of their stoichiometric coefficients divided by the product of the reactants raised to the power of their stoichiometric coefficients. This expression includes only gases and aqueous species.

Given the equation:

HC₃H₇CO₂ + NH₃ ⇄ C₃H₇CO₂⁻ + HNH₃⁺

This is an acid-base reaction that takes place in water, so Kc is:

$Kc=\frac{[C_{3}H_{7}CO_{2}^{-} ].[HNH_{3}^{+}]}{[HC_{3}H_{7}CO_{2}].[NH_{3}]}$

Answer 2

The expression for the equilibrium constant Kc is

$\rm Kc = \dfrac{[C_3H_7CO_2^-][HNH_3^+]}{[HC_3H_7CO_2][NH_3]}$

What is Kc?

Kc is the ratio of equilibrium product concentrations to equilibrium reactant concentrations.

The reaction

$HC_3H7CO_2 + NH_3 < = > C_3H_7CO_2^- + HNH_3+$

The equilibrium constant is the ratio of the products to the concentration of the products. The equilibrium constant  can be reached when the chemical reaction will reach the equilibrium. Once the reaction is in the equilibrium, then the concentration of every reactant can be measured.

Here, the acid base reaction is taking place

Thus, the expression for the equilibrium constant Kc is

$\rm Kc = \dfrac{[C_3H_7CO_2^-][HNH_3^+]}{[HC_3H_7CO_2][NH_3]}$

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