Consider the Daniell cell, for which the overall cell reaction is Zn(s)+Cu2+(aq)

Question

Consider the Daniell cell, for which the overall cell reaction is Zn(s)+Cu2+(aq)Zn2+(aq)+Cu(s) The concentrations of CuSO4 and ZnSO4 are 2.20×103 m and 1.10×103 m , respectively.

A)

Calculate E setting the activities of the ionic species equal to their molalities.

Express your answer to four significant figures and include the appropriate units.

B)

Calculate ±,ZnSO4 for the half-cell solutions using the Debye-Huckel limiting law.

Express your answer using three significant figures.

C)

Calculate ±,CuSO4 for the half-cell solutions using the Debye-Huckel limiting law.

Express your answer using three significant figures.

D)

Calculate E using the mean ionic activity coefficients determined in part (b) and part (c).

Express your answer to four significant figures and include the appropriate units.

Explanation / Answer

For the daniel cell

A) Using Nernst equation,

Ecell = Eo - 0.0592/n logK

        = (0.337 - (-0.763)) - 0.0592/2 log(1.1 x 10^-3/2.2 x 10^-3)

        = 0.435 V

B) Y[ZnSO4] = inv.log(-0.51 x 2^2 x sq/rt/(0.0044))/(1 + 3.3 x 0.6 x sq.rt.(0.0044))

                     = 0.759

C) Y[CuSO4] = inv.log(-0.51 x 2^2 x sq/rt/(0.0088))/(1 + 3.3 x 0.6 x sq.rt.(0.0088))

                     = 0.690

D) Ecell = 0.426 - 0.0592/2 log(0.759 x 1.1 x 10^-3/0.690 x 2.2 x 10^-3)

        = 0.443 V

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