A) Consider the following galvanic cell with a standard hydrogen electrode (S.H.

Question

A) Consider the following galvanic cell with a standard hydrogen electrode (S.H.E.) as the left electrode. Calculate the overall cell potential based on the indicated shorthand notation. Assume the temperature is 25° C. S.H.E. II Co2 (0.077 M) I Co

E for Co is -0.277...I know it's cathode but I am not sure how to calculate Ecell...i got 0.3099 and it was wrong.

B) Consider the following galvanic cell with a standard hydrogen electrode (S.H.E.) as the left electrode. Calculate the overall cell potential based on the indicated shorthand notation. Assume the temperature is 25° C. S.H.E. II Tl (0.075 M), Tl3 (0.805 M) I Pt

E for TI is 1.25

I am trying to figure out the E cell in Volts for Part A and Part B.

Any help is greatly appreciated. Thank you!

Explanation / Answer

Although we rarely use the standard hydrogen electrode (SHE) for routine analytical work, it is the reference electrode used to establish standard-state potentials for other half-reactions. The SHE consists of a Pt electrode immersed in a solution in which the activity of hydrogen ion is 1.00 and in which the fugacity of H2(g) is 1.00 (Figure 11.10). A conventional salt bridge connects the SHE to the indicator half-cell. The short hand notation for the standard hydrogen electrode is

Pt(s), H2(g, fH2 = 1.00) | H+(aq,aH+ = 1.00) ||

and the standard-state potential for the reaction

H+(aq) + e (ƒ1/2)H2(g)

is, by definition, 0.00 V at all temperatures. Despite its importance as the fundamental reference electrode against which we measure all other potentials, the SHE is rarely used because it is difficult to prepare and inconvenient to use.

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