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Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 3 Pb²+ (aq) + 2 Cr(s) →→ 3 Pb(s) + 2 Cr³¹ (aq)

Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 3 Pb²+ (aq) + 2 Cr(s) →→ 3 Pb(s) + 2 Cr³¹ (aq)

Chemistry
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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Solve 18.4 problem
Calculating Standard Potentials for Electrochemical cells from Standard Electrode Potentials of the half-Reactions: Look up the standard electrode Oxidation potentials for each half-reaction (Anode): in Table 18.1. Add the half-cell Reduction reactions together to obtain the (Cathode): NO; (aq) + 4H* (aq) + 3€ →→ NO(g) + 2 H₂O() Eº = 096V overall redox equation. Calculate Al(s) + NO (aq) + 4H* (aq) →→→ Al(aq) + NO(g) + 2H00) the standard cell potential by subtracting the electrode potential of the anode from the electrode potential of the cathode EE - E = 0.96 V-(-1.66V) = 2.62V AMS) AP (a)+30 E = -1.66V FOR PRACTICE 18.4 Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 3 Pb²+ (aq) + 2 Cr(s) 3 Pb(s) + 2 Cr³+ (aq) -
Transcribed Image Text:Calculating Standard Potentials for Electrochemical cells from Standard Electrode Potentials of the half-Reactions: Look up the standard electrode Oxidation potentials for each half-reaction (Anode): in Table 18.1. Add the half-cell Reduction reactions together to obtain the (Cathode): NO; (aq) + 4H* (aq) + 3€ →→ NO(g) + 2 H₂O() Eº = 096V overall redox equation. Calculate Al(s) + NO (aq) + 4H* (aq) →→→ Al(aq) + NO(g) + 2H00) the standard cell potential by subtracting the electrode potential of the anode from the electrode potential of the cathode EE - E = 0.96 V-(-1.66V) = 2.62V AMS) AP (a)+30 E = -1.66V FOR PRACTICE 18.4 Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 3 Pb²+ (aq) + 2 Cr(s) 3 Pb(s) + 2 Cr³+ (aq) -
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