Question

The equilibrium constant $\left(K_{c}\right)$ for the reaction $$ 2 \mathrm{HCl}(g) \rightleftarrows \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) $$ is $4.17 \times 10^{-34}$ at $25^{\circ} \mathrm{C}$. What is the equilibrium constant for the reaction $$ \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftarrows 2 \mathrm{HCl}(g) $$ at the same temperature?

Name: Problem 23, Chapter 15: Chemistry
Uploaded: 2020-07-01T16:28:23-08:00
Duration: 1 min 54 s
Channel: Kevin Zaborsky
Description: The equilibrium constant (Kc) for the reaction 2 HCl(g) ⇄H2(g)+Cl2(g) is 4.17 ×10^-34 at 25^∘ C. What is the equilibrium constant for the reaction H2(g)+Cl2(g) ⇄2 HCl(g) at the same temperature?

   The equilibrium constant $\left(K_{c}\right)$ for the reaction
$$
2 \mathrm{HCl}(g) \rightleftarrows \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)
$$
is $4.17 \times 10^{-34}$ at $25^{\circ} \mathrm{C}$. What is the equilibrium constant for the reaction
$$
\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftarrows 2 \mathrm{HCl}(g)
$$
at the same temperature?

Chemistry

Julia Burdge 1st Edition

Chapter 15, Problem 23

Instant Answer

Solved by Expert Kevin Zaborsky

07/01/2020

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17 \times 10^{-34}$ at $25^{\circ} \mathrm{C}$. Show more…

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The equilibrium constant $\left(K_{c}\right)$ for the reaction $$ 2 \mathrm{HCl}(g) \rightleftarrows \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) $$ is $4.17 \times 10^{-34}$ at $25^{\circ} \mathrm{C}$. What is the equilibrium constant for the reaction $$ \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftarrows 2 \mathrm{HCl}(g) $$ at the same temperature?

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Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible chemical reaction where the rate of the forward reaction equals the rate of the backward reaction. At this point, the concentrations of reactants and products remain constant over time, although both reactions continue to occur simultaneously.

Equilibrium Constant

The equilibrium constant (Kc) quantitatively expresses the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. It serves as a measure of the position of equilibrium, indicating how far a reaction proceeds before reaching equilibrium.

Reversing a Reaction

Reversing a chemical reaction involves switching the roles of the reactants and products. For the equilibrium constant, this means taking the reciprocal of the original constant. Understanding this concept is crucial as it shows how reaction direction influences the value of the equilibrium constant.

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