Which reaction has been chosen as the 'standard' against which every other reaction is measured?
A. Li+ + e– --> Li
B. F2 + 2e– --> 2F–
C. 2H+ + 2e– --> H2
D. O2 + 4H+ + 4e– ==> 2H2O
E. H2 + 2e– ==> 2H
It's C although you may get some argument from some BECAUSE, technically, the H^/H2 electrode is actually platinized Pt in a 1 M H^+ solution with H2 gas at 1 atm.
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To determine which reaction has been chosen as the 'standard' against which every other reaction is measured, we need to look at the standard reduction potentials of each reaction.
Standard reduction potentials are a way to measure the tendency of a species to gain electrons. The more positive the standard reduction potential, the greater the species' tendency to gain electrons and be reduced.
The 'standard' reaction chosen as the reference is the hydrogen electrode reaction, which is represented by Option E in the given choices:
E. H2 + 2e– ==> 2H
This reaction serves as the reference because it has a standard reduction potential of 0 volts. The standard reduction potential of the hydrogen electrode is defined as 0 volts by convention.
Therefore, the correct answer is E. H2 + 2e– ==> 2H.