**Electrochemical Cell Potential Calculation****Problem Statement:**What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is \(2.22 \times 10^{-3}\) atm, the H⁺ concentration is 1.38M, and the Cr³⁺ concentration is \(3.60 \times 10^{-4}\) M?**Chemical Reaction:**\[ 6.00 \text{H}^+(aq) + 2\text{Cr}(s) \rightarrow 3\text{H}_2(g) + 2\text{Cr}^{3+}(aq) \]**Answer:**\[ \text{Answer:} \, \, \square \, \text{V} \]**Spontaneity Query:**The cell reaction as written above is spontaneous for the concentrations given: \(\square\) (Dropdown selection: Yes/No).---**Explanation for Educational Context:**This problem involves calculating the cell potential of an electrochemical reaction at standard conditions (298K). Key data points provided include the pressures and concentrations of reactants and products involved in the redox reaction. The equation given represents a fundamental redox transformation between hydrogen ions, chromium metal, and their respective reduced and oxidized states.Students would typically use the Nernst equation to calculate the cell potential with the provided concentrations and partial pressures:\[ E = E^\circ - \frac{RT}{nF} \ln Q \]Where:- \( E \) is the cell potential.- \( E^\circ \) is the standard cell potential.- \( R \) is the universal gas constant.- \( T \) is the temperature in Kelvin.- \( n \) is the number of moles of electrons transferred.- \( F \) is the Faraday constant.- \( Q \) is the reaction quotient.Additionally, the problem includes a query on whether the reaction is spontaneous under the given conditions. The dropdown allows for evaluating if the calculated potential implies a spontaneous reaction.

Answered: Image /qna-images/answer/d2aaa9a8-983b-49a2-9e84-dac19ed8e325.jpg

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 2.22×10-3 atm, the H† concentration is 1.38M, and the Cr³+ concentration is 3.60×10-4M ? 6.00H*(aq) + 2Cr(s)- →3H2(g) + 2C1³*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 2.22×10-3 atm, the H† concentration is 1.38M, and the Cr³+ concentration is 3.60×10-4M ? 6.00H(aq) + 2Cr(s)- →3H2(g) + 2C1³(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

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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