The following reaction has an equilibrium constant, Kc equal to 1538 at 1800 . ^∘ C. 2 NO(g)+O2(

Name: Problem 36, Chapter 17: Chemistry
Uploaded: 2021-05-13T00:49:15-08:00
Duration: 47 s
Channel: Nicole Smina
Description: The following reaction has an equilibrium constant, Kc equal to 1538 at 1800 . ^∘ C. 2 NO(g)+O2( g) ⇌2 NO2( g) Calculate the equilibrium constant, Kc, for the reverse equation.

step 1 So if the equilibrium constant for the forward reaction is 1 ,538, for the reverse, it's 1 over

Question

The following reaction has an equilibrium constant, $K_{\mathrm{c}}$ equal to 1538 at $1800 .{ }^{\circ} \mathrm{C}$. $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$$ Calculate the equilibrium constant, $K_{c}$, for the reverse equation.

   The following reaction has an equilibrium constant, $K_{\mathrm{c}}$ equal to 1538 at $1800 .{ }^{\circ} \mathrm{C}$.
$$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$$
Calculate the equilibrium constant, $K_{c}$, for the reverse equation.

Chemistry

Kenneth W. Whitten,… 10th Edition

Chapter 17, Problem 36

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Solved by Expert Nicole Smina

05/13/2021

Step 1

Step 1: The equilibrium constant for the forward reaction is given as $K_{c} = 1538$. Show more…

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The following reaction has an equilibrium constant, $K_{\mathrm{c}}$ equal to 1538 at $1800 .{ }^{\circ} \mathrm{C}$. $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$$ Calculate the equilibrium constant, $K_{c}$, for the reverse equation.

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Key Concepts

Equilibrium Constant (Kc)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is a measure of the extent to which a reaction proceeds and provides insight into the reaction's directionality under specific conditions.

Reversing a Reaction and Its Equilibrium Constant

When the direction of a chemical reaction is reversed, the equilibrium constant for the new reaction is the reciprocal of the original equilibrium constant. This inversion occurs because the roles of the reactants and products are switched, thereby reversing the concentration ratio.

Application of the Reciprocal Relationship

In practice, if the equilibrium constant for a forward reaction is known, the equilibrium constant for the reverse reaction can be easily determined by taking the reciprocal. This concept is fundamental in analyzing and understanding chemical equilibria and reaction dynamics.

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