Which of the following reductions will occur in the presence of H2 gas under standard conditions

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Which of the following reductions will occur in the presence...

Which of the following reductions will occur in the presence of $\mathrm{H}_{2}$ gas under standard conditions?
a. $A g^{+}$ to $A g$
b. $\mathrm{Mg}^{2+}$ to $\mathrm{Mg}$
c. $\mathrm{Cu}^{2+}$ to $\mathrm{Cu}$
d. $\mathrm{Cd}^{2+}$ to $\mathrm{Cd}$

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Key Concepts

Redox Reaction Spontaneity

Determining the spontaneity of a redox reaction involves comparing the standard reduction potentials of the two half-reactions. A reaction is spontaneous when the overall cell potential (difference between the reduction and oxidation potentials) is positive. This concept is fundamental in predicting whether a reducing agent, such as hydrogen gas, can drive the reduction of another species under standard conditions.

Standard Reduction Potentials

This concept refers to the measured tendency of a chemical species to acquire electrons and thus be reduced. It is expressed as a voltage relative to the standard hydrogen electrode, which allows the prediction of whether a redox reaction (electron transfer reaction) will occur spontaneously under standard conditions.

Electrochemical Series

The electrochemical series is an arrangement of elements and compounds according to their standard reduction potentials. It helps in comparing the tendency of different species to be reduced or oxidized, and it is crucial in determining which redox reactions are thermodynamically favorable based on the relative positions of the half-reactions.

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