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The standard half-cell potential for the reaction O2(g)+4H+(aq)+4e−→2H2O(l) is +1.229 V at 298.15 K. The aO2 = 1.00...

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Chemistry

The standard half-cell potential for the reaction
O2(g)+4H+(aq)+4e−→2H2O(l) is+1.229 V at 298.15 K.
The aO2 = 1.00 assuming that the aH+ is equal tothe molality.

Part A

Calculate E for a 0.100-molal solution of H2SO4 foraO2 = 1.00 assuming that the aH+ isequal to the molality.

Part B

Calculate E for a 0.100-molal solution of H2SO4 foraO2= 1.00 using the measured mean ionic activitycoefficient for this concentration from the data tables in thetextbook.

Part C

How large is the relative error if the concentrations, ratherthan the activities, are used?

Answer & Explanation Solved by verified expert
3.6 Ratings (372 Votes)
To find the electrochemical potential of a cell we use the Nerstequation which is given asQreaction quotient or simply it can be replaced with K theequilibrium constantn number    See Answer
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