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

step 1 There's a couple ways to answer this question. We could look up the reduction potential for the

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

Which of the following oxidations will occur in the presence of $\mathrm{H}_{2}$ gas under standard conditions?
a. $\mathrm{Zn}^{2+}$ to $\mathrm{Zn}$
b. $\mathrm{Fe}^{2+}$ to $\mathrm{Fe}^{3+}$
c. $\mathrm{Cr}(\mathrm{OH})_{3}$ to $\mathrm{CrO}_{4}^{2-}$
d. Ni to Ni $^{2+}$

Key Concepts

Hydrogen Electrode as a Reference

The hydrogen electrode, with its standard potential set at 0 V, serves as a reference point for measuring and comparing the potential of other half-reactions. Understanding its role helps in evaluating whether a given species will be oxidized or reduced when paired with hydrogen gas in an electrochemical context.

Reaction Spontaneity and Gibbs Free Energy

The spontaneity of a redox reaction under standard conditions is determined by the overall cell potential, which is related to the Gibbs free energy change. A positive cell potential implies that the reaction will proceed spontaneously, linking electrochemical potentials directly to thermodynamic favorability.

Redox Reactions

Redox reactions involve the transfer of electrons between chemical species, where one species undergoes oxidation (loss of electrons) and the other undergoes reduction (gain of electrons). This fundamental concept is essential in understanding how and why electronic changes occur in chemical reactions and in predicting the direction of electron flow.

Standard Electrode Potentials

Standard electrode potentials provide a measure of the tendency of a chemical species to be reduced, given under standard conditions. By comparing these potentials, one can predict which half-reaction will proceed as oxidation and which as reduction, thereby determining the spontaneity of the reaction.

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