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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.101QE: At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction...
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Question
Solve 18.4 problem
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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