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Consider the cell Zn(s)|ZnCl2(0.005 mol kg-1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s)+Zn(s)->2Hg(l)+2Cl-(aq)+Zn2+(aq). The cell potential is 1.2272 V, E0(Zn2+,Zn)=-0.7628V, and E0(Hg2Cl2,Hg)=+0.2676V. Calculate the ∆ r G 0 , ∆ r G and

Consider the cell Zn(s)|ZnCl2(0.005 mol kg-1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s)+Zn(s)->2Hg(l)+2Cl-(aq)+Zn2+(aq). The cell potential is 1.2272 V, E0(Zn2+,Zn)=-0.7628V, and E0(Hg2Cl2,Hg)=+0.2676V. Calculate the ∆ r G 0 , ∆ r G and

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 35QRT
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Consider the cell Zn(s)|ZnCl2(0.005 mol kg-1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s)+Zn(s)->2Hg(l)+2Cl-(aq)+Zn2+(aq). The cell potential is 1.2272 V, E0(Zn2+,Zn)=-0.7628V, and E0(Hg2Cl2,Hg)=+0.2676V. Calculate the ∆ r G 0 , ∆ r G and K e q .

 

Question 7 options:

 

A. -202.23 kJ.mol-1; 222.85 kJ.mol-1; 6.21x1032

 

B. -198.84 kJ.mol-1; 236.81 kJ.mol-1; 7.11x1034

 

C. -182.23 kJ.mol-1; 256.22 kJ.mol-1; 5.66x1033

 

D. -190.34 kJ.mol-1; 232.42 kJ.mol-1; 6.62x1031 

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