Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox is spontaneous or nonspontaneous Au+(aq)+e-→Au(s) E0=1.69V N2O(g)+2H+(aq)+2e-→N2(g) +H2O(l) E0=1.77V Cr3+(aq)+3e-→Cr(s) E0= -0.74V Half-Reactions E0cell Spontaneity ( Spontaneous or Nonspontaneous) N2(g)+H2O(l)+2Au+(aq)→N2O(g)+2H+(aq)+2Au(s) _ _ 3N2O(g)+6H+(aq)+2Cr(s)→3N2(g)+3H2O(l)+2Cr3+(aq) _ _ 3Au+(aq)+Cr(s)→Cr3+(aq)+3Au(s) _ _
Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox is spontaneous or nonspontaneous Au+(aq)+e-→Au(s) E0=1.69V N2O(g)+2H+(aq)+2e-→N2(g) +H2O(l) E0=1.77V Cr3+(aq)+3e-→Cr(s) E0= -0.74V Half-Reactions E0cell Spontaneity ( Spontaneous or Nonspontaneous) N2(g)+H2O(l)+2Au+(aq)→N2O(g)+2H+(aq)+2Au(s) _ _ 3N2O(g)+6H+(aq)+2Cr(s)→3N2(g)+3H2O(l)+2Cr3+(aq) _ _ 3Au+(aq)+Cr(s)→Cr3+(aq)+3Au(s) _ _
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.143QP: Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this...
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Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox is spontaneous or nonspontaneous
Au+(aq)+e-→Au(s) E0=1.69V
N2O(g)+2H+(aq)+2e-→N2(g) +H2O(l) E0=1.77V
Cr3+(aq)+3e-→Cr(s) E0= -0.74V
| Half-Reactions | E0cell | Spontaneity ( Spontaneous or Nonspontaneous) |
| N2(g)+H2O(l)+2Au+(aq)→N2O(g)+2H+(aq)+2Au(s) | _ | _ |
| 3N2O(g)+6H+(aq)+2Cr(s)→3N2(g)+3H2O(l)+2Cr3+(aq) | _ | _ |
|
3Au+(aq)+Cr(s)→Cr3+(aq)+3Au(s) |
_ | _ |
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