### Equilibrium Constant Calculations#### Given the Two Reactions:1. \( \text{H}_2\text{S(aq)} \rightleftharpoons \text{HS}^-(\text{aq}) + \text{H}^+(\text{aq}), \quad K_1 = 9.46 \times 10^{-8} \)2. \( \text{HS}^-(\text{aq}) \rightleftharpoons \text{S}^{2-}(\text{aq}) + \text{H}^+(\text{aq}), \quad K_2 = 1.31 \times 10^{-19} \)**What is the equilibrium constant \( K_{\text{final}} \) for the following reaction?**\[ \text{S}^{2-}(\text{aq}) + 2\text{H}^+(\text{aq}) \rightleftharpoons \text{H}_2\text{S(aq)} \]\[ K_{\text{final}} = \text{[Select]} \]---#### Given the Two Reactions:3. \( \text{PbCl}_2\text{(aq)} \rightleftharpoons \text{Pb}^{2+}(\text{aq}) + 2\text{Cl}^-(\text{aq}), \quad K_3 = 1.81 \times 10^{-10} \)4. \( \text{AgCl(s)} \rightleftharpoons \text{Ag}^+(\text{aq}) + \text{Cl}^-(\text{aq}), \quad K_4 = 1.21 \times 10^{-4} \)**What is the equilibrium constant \( K_{\text{final}} \) for the following reaction?**\[ \text{PbCl}_2(\text{aq}) + 2\text{Ag}^+(\text{aq}) \rightleftharpoons 2\text{AgCl(s)} + \text{Pb}^{2+}(\text{aq}) \]\[ K_{\text{final}} = \text{[Select]} \]---### Explanation of Reactions and DiagramsFor the given reactions, you are asked to determine the equilibrium constants, \( K_{\text{final}} \), for

Answer:For any reaction, equilibrium constant is equal to the ratio of molar concentration of…

Given the two reactions 1. H₂S(aq) = HS (aq) + H*(aq), K₁ = 9.46x10-8, and 2. HS¯(aq) = S² (aq)+H*(aq), K₂ = 1.31×10-¹⁹, what is the equilibrium constant Kfinal for the following reaction? S²¯(aq)+2H*(aq)=H₂S(aq) Kfinal = [Select] Given the two reactions 3. PbCl₂(aq) = Pb2+(aq)+2Cl¯(aq), K3 = 1.81×10-10, and 4. AgCl(aq) = Agt(aq) +CI (aq), K4 = 1.21×10-4, what is the equilibrium constant Kfinal for the following reaction? PbCl₂(aq) + 2Ag+(aq): = 2AgCl(aq) + Pb2+(aq) Kfinal = [Select]

Given the two reactions 1. H₂S(aq) = HS (aq) + H(aq), K₁ = 9.46x10-8, and 2. HS¯(aq) = S² (aq)+H(aq), K₂ = 1.31×10-¹⁹, what is the equilibrium constant Kfinal for the following reaction? S²¯(aq)+2H*(aq)=H₂S(aq) Kfinal = [Select] Given the two reactions 3. PbCl₂(aq) = Pb2+(aq)+2Cl¯(aq), K3 = 1.81×10-10, and 4. AgCl(aq) = Agt(aq) +CI (aq), K4 = 1.21×10-4, what is the equilibrium constant Kfinal for the following reaction? PbCl₂(aq) + 2Ag+(aq): = 2AgCl(aq) + Pb2+(aq) Kfinal = [Select]

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

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Question

### Equilibrium Constant Calculations

#### Given the Two Reactions:

1. \( \text{H}_2\text{S(aq)} \rightleftharpoons \text{HS}^-(\text{aq}) + \text{H}^+(\text{aq}), \quad K_1 = 9.46 \times 10^{-8} \)
2. \( \text{HS}^-(\text{aq}) \rightleftharpoons \text{S}^{2-}(\text{aq}) + \text{H}^+(\text{aq}), \quad K_2 = 1.31 \times 10^{-19} \)

**What is the equilibrium constant \( K_{\text{final}} \) for the following reaction?**

\[ \text{S}^{2-}(\text{aq}) + 2\text{H}^+(\text{aq}) \rightleftharpoons \text{H}_2\text{S(aq)} \]

\[ K_{\text{final}} = \text{[Select]} \]

---

#### Given the Two Reactions:

3. \( \text{PbCl}_2\text{(aq)} \rightleftharpoons \text{Pb}^{2+}(\text{aq}) + 2\text{Cl}^-(\text{aq}), \quad K_3 = 1.81 \times 10^{-10} \)
4. \( \text{AgCl(s)} \rightleftharpoons \text{Ag}^+(\text{aq}) + \text{Cl}^-(\text{aq}), \quad K_4 = 1.21 \times 10^{-4} \)

**What is the equilibrium constant \( K_{\text{final}} \) for the following reaction?**

\[ \text{PbCl}_2(\text{aq}) + 2\text{Ag}^+(\text{aq}) \rightleftharpoons 2\text{AgCl(s)} + \text{Pb}^{2+}(\text{aq}) \]

\[ K_{\text{final}} = \text{[Select]} \]

---

### Explanation of Reactions and Diagrams

For the given reactions, you are asked to determine the equilibrium constants, \( K_{\text{final}} \), for

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