**47. Consider the reaction:**\[ \text{NH}_4\text{HS}(s) \rightleftharpoons \text{NH}_3(g) + \text{H}_2\text{S}(g) \]At a certain temperature, \( K_c = 8.5 \times 10^{-3} \). A reaction mixture at this temperature containing solid NH₄HS has \([\text{NH}_3] = 0.166 \, \text{M}\) and \([\text{H}_2\text{S}] = 0.166 \, \text{M}\). Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?**Missed This?** Read Section 16.7; Watch KCV 16.7, IWE 16.7

Given equilibrium is NH4HS(s) <----> NH3(g) + H2S(g) Equilibrium constant , Kc = 8.5×10-3 A…

47. Consider the reaction: MISSED THIS? Read Section 16.7; Watch KCV 16.7, WE 16.7 NH,HS(s) = NH3(8) + H2S(g) At a certain temperature, K̟ = 8.5 × 10-³. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

47. Consider the reaction: MISSED THIS? Read Section 16.7; Watch KCV 16.7, WE 16.7 NH,HS(s) = NH3(8) + H2S(g) At a certain temperature, K̟ = 8.5 × 10-³. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

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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