Use the following two half-reactions to write balanced net ionic equations for one spontaneous reaction and one non-spontaneous reaction. State the standard cell potential for each reaction: N2O(g) + 2H+(aq) + 2e– —> N2 (g) + H2O(l) (E° = 1.770 V) Cul(s) + e– —> Cu(s) + I–(aq) (E° = -0.185 V)
Use the following two half-reactions to write balanced net ionic equations for one spontaneous reaction and one non-spontaneous reaction. State the standard cell potential for each reaction: N2O(g) + 2H+(aq) + 2e– —> N2 (g) + H2O(l) (E° = 1.770 V) Cul(s) + e– —> Cu(s) + I–(aq) (E° = -0.185 V)
Chapter18: Introduction To Electrochemistry
Section: Chapter Questions
Problem 18.18QAP
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Use the following two half-reactions to write balanced net ionic equations for one spontaneous reaction and one non-spontaneous reaction. State the standard cell potential for each reaction:
N2O(g) + 2H+(aq) + 2e– —> N2 (g) + H2O(l) (E° = 1.770 V)
Cul(s) + e– —> Cu(s) + I–(aq) (E° = -0.185 V)
State the oxidizing agent and the reducing agent in a lead-acid battery that is
a) discharging
b) recharging
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