esoutce from Cengage Learning - Google Chrome om/ilrn/takeAssignment/takeCovalen

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esoutce from Cengage Learning - Google Chrome om/ilrn/takeAssignment/takeCovalentActivity do?locator-assignment-take&takeAssignmentSessionLocator-assignment-take; Review Topics] Use the References to access important values if needed for this question. y change for the following reaction at 25 c, when [Zn2]-8.66x103 M and [Sa2]- 1.16 M, is 132 kJ Zn2+( 8.66x 10-3 M)-Sn(s)-- Zn(s)- Sn2+( 1.16 M) G 132 kJ What is the cell potential for the reaction as written under these conditions? Answer Would this reaction be spontaneous in the forward or the reverse direction? Retry Entire Group 9 more group attempts remaining Submit Answer

Explanation / Answer

Zn2+(aq) + Sn(s) ---> Zn(s) + Sn2+ (aq) : G = 132 kJ

We know that G = -nFEo

Where n = number of electrons transferred = change in oxidation of Sn = 2 - 0 = 2

F = Faraday = 96500 C

Eo = cell potential = ?

G = 132 kJ x(103 J/kJ) = 132x103 J

Plug the values we get Eo = -(G ) / (nF)

= -0.68 V

Since the value of Eo is negative it is non-spontaneous in forward direction.

It is spontaneous in reverse direction.

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