Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential `(E^(@))` of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniel cell in which zinc goes into solution and copper gets deposited.
For the cell: Pt `|H_(2)(0.4"atm")H^(+)(pH=1)||H^(+)(pH=2)|H_(2)(0.1"atm")|` Pt, the measured potential at `25^(@)C` is:
[Given: 2.303RT/F=0.06V, log 2=0.3]
A. `-0.1V`
B. `-0.5V`
C. `-0.042V`
D. `-0.035V`
