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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H₂ pressure is 2.04x10-3 bar, the H+ concentration is 1.43 M, and the Al³+ concentration is 6.14x10-4 M ? 6H+ (aq) + 2Al(s)—3H₂(g) + 2Al³+ (aq) Answer: v The cell reaction as written above is product-favored (spontaneous) for the concentrations given: Submit Show Approach Hide Tutor Steps

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H₂ pressure is 2.04x10-3 bar, the H+ concentration is 1.43 M, and the Al³+ concentration is 6.14x10-4 M ? 6H+ (aq) + 2Al(s)—3H₂(g) + 2Al³+ (aq) Answer: v The cell reaction as written above is product-favored (spontaneous) for the concentrations given: Submit Show Approach Hide Tutor Steps

Principles of Instrumental Analysis
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter22: An Introduction To Electroanalytical Chemistry
Section: Chapter Questions
Problem 22.7QAP: Calculate the theoretical potential of each of the following cells. Is the cell reaction spontaneous...
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Approach The nonstandard potential for a cell can be related to the standard cell potential using the Nernst equation: Ecell = Ecell RT nF x In Q Where R = 8.314 J K¹ mol-¹ and F = 96.485 J V-¹ mol-¹ At 298 K, this RT/F combine to give, 0.0257 V Ecell = Ecell x In Q n When one of the reactants or products is a gas, its pressure is used to calculate the reaction quotient, Q. Concentrations are used in moles per liter. Pressures of gas-phase species are used in units of bars. Step 1. Write the anode and cathode half-reactions and determine n. Step 2. Calculate Eºcell. Step 3. Calcuate Q. Step 4. Calculate Ecell under these nonstandard conditions.
Transcribed Image Text:Approach The nonstandard potential for a cell can be related to the standard cell potential using the Nernst equation: Ecell = Ecell RT nF x In Q Where R = 8.314 J K¹ mol-¹ and F = 96.485 J V-¹ mol-¹ At 298 K, this RT/F combine to give, 0.0257 V Ecell = Ecell x In Q n When one of the reactants or products is a gas, its pressure is used to calculate the reaction quotient, Q. Concentrations are used in moles per liter. Pressures of gas-phase species are used in units of bars. Step 1. Write the anode and cathode half-reactions and determine n. Step 2. Calculate Eºcell. Step 3. Calcuate Q. Step 4. Calculate Ecell under these nonstandard conditions.
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H₂ pressure is 2.04×10-3 bar, the H+ concentration is 1.43 M, and the Al³+ concentration is 6.14x10-4 M ? 6H+ (aq) + 2Al(s)—3H₂(g) + 2Al³+ (aq) Answer: V The cell reaction as written above is product-favored (spontaneous) for the concentrations given: Submit Show Approach Hide Tutor Steps
Transcribed Image Text:What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H₂ pressure is 2.04×10-3 bar, the H+ concentration is 1.43 M, and the Al³+ concentration is 6.14x10-4 M ? 6H+ (aq) + 2Al(s)—3H₂(g) + 2Al³+ (aq) Answer: V The cell reaction as written above is product-favored (spontaneous) for the concentrations given: Submit Show Approach Hide Tutor Steps
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