A student wishes to determine the chlorideion concentration in a water sample at 25°C using a galvanic cell constructed with agraphite electrode and a half-cell of AgCl(s)+ e- → Ag(s) + Cl-(aq) E°red = 0.2223 V And acopper electrode with 0.500 M Cu²+ as thesecond half cell Cu²+(aq) + 2 e- → Cu(s)E°red= 0.337 V The measured cell potentialwhen the water sample was placed into thesilver side of the cell was O.0761 V. Giventhe standard cell potential for this cell is0.115 V, what is the value of the standardfree energy (in kJ) for this reaction?

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0.115 V, what is the value of the standard free energy (in kJ) for this reaction?

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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Question

A student wishes to determine the chloride
ion concentration in a water sample at 25
°C using a galvanic cell constructed with a
graphite electrode and a half-cell of AgCl(s)
+ e- → Ag(s) + Cl-(aq) E°red = 0.2223 V And a
copper electrode with 0.500 M Cu²+ as the
second half cell Cu²+(aq) + 2 e- → Cu(s)
E°red= 0.337 V The measured cell potential
when the water sample was placed into the
silver side of the cell was O.0761 V. Given
the standard cell potential for this cell is
0.115 V, what is the value of the standard
free energy (in kJ) for this reaction?

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As it is a cell reaction the formula to calculate the standard free energy change is this-

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