**Electrochemical Cell Calculations****Part 1: Balanced Chemical Equation**Write the balanced chemical equation that occurs in an electrochemical cell that employs these half-reactions. Include states of matter.\[ \text{O}_2(g) + 2\text{H}_2\text{O}(l) + 2\text{Ca}(s) \rightarrow 4\text{OH}^-(aq) + 2\text{Ca}^{2+}(aq) \]**Part 2: Work Calculation Under Standard Conditions**Calculate the maximum amount of work produced by this cell under standard conditions. Ensure the sign indicates the relationship of the work between the cell and the surroundings.Work: \(-1261.6 \, \text{kJ}\)**Part 3: Work Calculation Under Non-standard Conditions**Calculate the maximum amount of work produced by the cell when the partial pressure of \(\text{O}_2\) is 0.2050 atm, the pH is 7.167, and the concentration of \(\text{Ca}^{2+}\) is 0.0140 M.Work: \(-1434.1 \, \text{kJ}\) **Standard Reduction Potentials**Consider the following standard reduction potentials:1. For the reduction of oxygen: \[ \text{O}_2(g) + 2\text{H}_2\text{O}(l) + 4e^- \rightarrow 4\text{OH}^-(aq) \quad E^\circ = 0.401 \, \text{V} \]2. For the reduction of calcium ions: \[ \text{Ca}^{2+}(aq) + 2e^- \rightarrow \text{Ca}(s) \quad E^\circ = -2.868 \, \text{V} \]These equations represent the standard reduction potentials (\(E^\circ\)) for different reactions, measured in volts. The positive value indicates a greater tendency for the substance to gain electrons and be reduced, while a negative value indicates a lower tendency.

Part 1 and part 2 is already done and correct. Providing you with the answer solution for part 3. According to the question, The partial pressure of the O2 is given by (P) =0.2050 The pH is given by = 7.167 The concentration of the Ca2+ is given by = 0.0140 MThe cell reaction for the given question can be written as, Anode reaction [Ca → Ca2+ + 2e-] ×2 Cathode reaction O2 + 2H2O + 4e- → 4OH-Overall reaction 2Ca + O2 + 2H2O → 2Ca2+ + 4OH- The electrode potential of the cell can also be written as, E°Reduction(cathode) (OH-,O2|Pt) = 0.401 V E°Reduction (anode) (Ca2+|Ca) = -2.868 V E°cell = E°red(cathode) -E°red(anode) E°cell = 0.401 -(-2.868) = 0.401+2.868 = 3.269 V The emf of the cell (Ecell ) can also be calculated by, Ecell =E°cell - 0.059nlog Q where Q=Ca2+2 OH-4PO2 As the pH = 7.167 pOH = 14 - pH=14 - 7.167=6.833 log [OH-] = -6.833 [OH-] = antilog -6.833=1.5×10-7 substituting all values we get, Q=0.01402 1.5×10-70.2050=4.8×10-31 Substitute all the values in the emf cell of reaction, Ecell = 3.269 - 0.0594log 4.8×10-31=3.269 -−0.447=3.716 V The maximum amount of work done can be calculated by, ∆G = -nFEcell where, n = number of electrons used = 4 F = Faradays Constant = 96485 F Ecell = 3.716 V Substitute the all values we get, ∆G = -4×96485×3.716=-1434153.04 J=-1434153.04 1000kJ=-1434.15 kJor=-1434.15≃-1434 kJ The required maximum amount of work done is found to be 1434 kJ

Science

Chemistry

Write the balanced chemical equation that occurs in an electrochemical cell that employs these half-reactions. Include states of matter. X Part 2 X He O₂(g) + 2H₂O(1) +2Ca(s). -1261.6 Part 3 (aq). ỗ kJ Calculate the maximum amount of work produced by this cell under standard conditions. Make sure the sign indicates the relationship of the work between the cell and the surroundings. 40H(aq) + 2Ca²+ (aq) Feedback Feedback Calculate the maximum amount of work produced by the cell when the partial pressure of O2 is 0.2050 atm, the pH is 7.167, and the concentration of Ca2+ is 0.0140 M. X-1434.1 kj

Write the balanced chemical equation that occurs in an electrochemical cell that employs these half-reactions. Include states of matter. X Part 2 X He O₂(g) + 2H₂O(1) +2Ca(s). -1261.6 Part 3 (aq). ỗ kJ Calculate the maximum amount of work produced by this cell under standard conditions. Make sure the sign indicates the relationship of the work between the cell and the surroundings. 40H(aq) + 2Ca²+ (aq) Feedback Feedback Calculate the maximum amount of work produced by the cell when the partial pressure of O2 is 0.2050 atm, the pH is 7.167, and the concentration of Ca2+ is 0.0140 M. X-1434.1 kj

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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231. Subject :- Chemistry
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