**Chem 1B****Chapter-17 Tutorial Worksheet**---**Reduction Potentials of Selected Substances:**- **PbO₂ + HSO₄⁻ + 3H⁺ + 2e⁻ → PbSO₄ + 2H₂O;** \( \varepsilon^\circ = -1.68 \, \text{V} \)- **MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 2H₂O;** \( \varepsilon^\circ = 1.51 \, \text{V} \)- **Au³⁺ + 3e⁻ → Au;** \( \varepsilon^\circ = 1.50 \, \text{V} \)- **Cl₂ + 2e⁻ → 2Cl⁻;** \( \varepsilon^\circ = 1.36 \, \text{V} \)- **Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O;** \( \varepsilon^\circ = 1.23 \, \text{V} \)- **MnO₄⁻ + 4H⁺ + 3e⁻ → MnO₂ + 2H₂O;** \( \varepsilon^\circ = 1.23 \, \text{V} \)- **O₂ + 4H⁺ + 4e⁻ → 2H₂O;** \( \varepsilon^\circ = 1.23 \, \text{V} \)- **Br₂ + 2e⁻ → 2Br⁻;** \( \varepsilon^\circ = 1.09 \, \text{V} \)- **NO₃⁻ + 4H⁺ + 3e⁻ → NO + 2H₂O;** \( \varepsilon^\circ = 0.96 \, \text{V} \)- **2Hg²⁺ + 2e⁻ → Hg₂²⁺;** \( \varepsilon^\circ = 0.92 \, \text{V} \)- **Exercise on Standard Electrode Potentials**In this exercise, you are tasked to calculate the standard cell potential (\(E^\circ_{\text{cell}}\)) for each of the given redox reactions using the Table of Standard Electrode Potentials (refer to Appendix L, page 1251), and predict whether the reactions are spontaneous or non-spontaneous.**Reactions:**(a) \( \text{Au}(s) + \text{NO}_3^-(aq) + 4\text{H}^+(aq) \rightarrow \text{Au}^{3+}(aq) + \text{NO}(g) + 2\text{H}_2\text{O}(l) \)(b) \( \text{Cu}(s) + 2\text{Fe}^{2+}(aq) \rightarrow \text{Cu}^{2+}(aq) + \text{Fe}(s) \)(c) \( 2\text{Fe}^{3+}(aq) + 2\text{I}^-(aq) \rightarrow \text{I}_2(aq) + 2\text{Fe}^{2+}(aq) \)(d) \( \text{Zn(OH)}_2(s) + 4\text{NH}_3(aq) \rightarrow [\text{Zn(NH}_3\text{)}_4]^{2+}(aq) + 2\text{OH}^-(aq) \)**Instructions:**1. Use the standard reduction potentials from the table provided to find the \(E^\circ_{\text{cell}}\) for each reaction.2. Remember, a positive \(E^\circ_{\text{cell}}\) value indicates a spontaneous reaction, while a negative value indicates a non-spontaneous reaction.**Analysis:**- For each reaction, write down the two half-reactions (oxidation and reduction).- Calculate the \(E^\circ_{\text{cell}}\) using the formula: \[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]- Use the calculated potential to determine spontaneity. Engage with this exercise to deepen your understanding of electrochemical cells and redox reaction spontaneity.

We have to calculate the Ecell for each of the following given reactions and predict the whether…

Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);

Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H(aq) → Au³(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);

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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