Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox is spontaneous or nonspontaneousAu+(aq)+e-→Au(s) E0=1.69VN2O(g)+2H+(aq)+2e-→N2(g) +H2O(l) E0=1.77VCr3+(aq)+3e-→Cr(s) E0= -0.74VHalf-ReactionsE0cellSpontaneity ( 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)__

The reaction which involves both oxidation and reduction is called as the redox reaction. The…

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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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Use the following half-reactions to calculate the E⁰_cell 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^-→N_2(g) +H₂O_(l) E⁰=1.77V

Cr³⁺_(aq)+3e^-→Cr_(s) E⁰= -0.74V

Half-Reactions	E⁰_cell	Spontaneity ( Spontaneous or Nonspontaneous)
N_2(g)+H₂O_(l)+2Au⁺_(aq)→N₂O_(g)+2H⁺_(aq)+2Au_(s)	_	_
3N₂O_(g)+6H⁺_(aq)+2Cr_(s)→3N_2(g)+3H₂O_(l)+2Cr³⁺_(aq)	_	_
3Au⁺_(aq)+Cr_(s)→Cr³⁺_(aq)+3Au_(s)	_	_

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