Given the following reaction: Cr2O72- (aq) + I- (aq) ® Cr3+ (aq) + I2 (s) a) Balance the above reactions under acidic conditions: b) If this balanced reaction was a voltaic cell, write down equations representing the anode half-reaction and the cathode half-reaction. c) If the Standard Reduction Potential for the half-reaction involving Cr2O72- (aq) is +1.33 V and that for the half-reaction involving I2 is +0.535V, determine E°cell . Also calculate the equilibrium constant and ΔG° for the reaction.
Given the following reaction: Cr2O72- (aq) + I- (aq) ® Cr3+ (aq) + I2 (s) a) Balance the above reactions under acidic conditions: b) If this balanced reaction was a voltaic cell, write down equations representing the anode half-reaction and the cathode half-reaction. c) If the Standard Reduction Potential for the half-reaction involving Cr2O72- (aq) is +1.33 V and that for the half-reaction involving I2 is +0.535V, determine E°cell . Also calculate the equilibrium constant and ΔG° for the reaction.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 90AP: Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode...
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Given the following reaction:
Cr2O72- (aq) + I- (aq) ® Cr3+ (aq) + I2 (s)
a) Balance the above reactions under acidic conditions:
b) If this balanced reaction was a voltaic cell, write down equations representing the anode half-reaction and the cathode half-reaction.
c) If the Standard Reduction Potential for the half-reaction involving Cr2O72- (aq) is +1.33 V and that for the half-reaction involving I2 is +0.535V, determine E°cell .
Also calculate the equilibrium constant and ΔG° for the reaction.
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