### Calculating the Equilibrium Constant (K_eq)To determine the value of the equilibrium constant (\(K_{eq}\)) for the given reaction, we use the equilibrium concentrations provided.The reaction in question is:\[ 2 \text{H}_2\text{S}_{(g)} \rightleftharpoons 2 \text{H}_{2(g)} + \text{S}_{2(g)} \]The equilibrium concentrations are:- \([\text{H}_2\text{S}] = 0.25 \, \text{M}\)- \([\text{H}_2] = 0.88 \, \text{M}\)- \([\text{S}_2] = 0.44 \, \text{M}\)### Steps to Calculate \(K_{eq}\)1. **Write the expression for the equilibrium constant (\(K_{eq}\)):** \[ K_{eq} = \frac{[\text{H}_2]^2 [\text{S}_2]}{[\text{H}_2\text{S}]^2} \]2. **Substitute the equilibrium concentrations into the expression:** \[ K_{eq} = \frac{(0.88)^2 \cdot (0.44)}{(0.25)^2} \]3. **Perform the calculations:** - Calculate the numerator: \((0.88)^2 \times (0.44) = 0.7744 \times 0.44 = 0.340736\) - Calculate the denominator: \((0.25)^2 = 0.0625\) \[ K_{eq} = \frac{0.340736}{0.0625} \approx 5.45 \]### ResultThe value of the equilibrium constant (\(K_{eq}\)) for the reaction is approximately **5.45**.### Explanation of Diagrams and GraphsThere are no diagrams or graphs included in this content. The text focuses on presenting and solving a chemical equilibrium problem through mathematical expressions and equilibrium concentrations.

The question is based on the concept of chemical equilibrium. We have to calculate EQUILIBRIUM…

Answered: Calculate the value of K, in the…

Calculate the value of K, in the following reaction if the equilibrium concentrations are [H,S] = 0.25 M, [H,] = 0.88 M, [S,] = 0.44M. 2 H,Se = 2 Hzie) '2(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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