Final answer:
Doubling the coefficients in the redox reaction affects the voltaic cell by squaring InQ and Q, doubling n, while E and Eo remain unaffected.
Step-by-step explanation:
When considering how doubling the coefficients in a redox reaction affects a voltaic cell under nonstandard conditions, we need to look at each element involved in the reaction:
- InQ: The reaction quotient, Q, is dependent on the concentration of the reactants and products. Doubling the coefficients will square the contribution of each reactant and product to Q since they are raised to the power of their respective coefficients in the expression for Q.
- Eo: The standard electrode potential (Eo) is not affected by the stoichiometric coefficients of the reaction. This value is a property of the half-reactions and not dependent on the amount of substance involved.
- E: The cell potential (E) under nonstandard conditions is also not directly affected by the stoichiometric coefficients of the reaction, as it is calculated from the Nernst equation, which incorporates Q but not the coefficients directly.
- n: The number of electrons transferred in the reaction, n, will be doubled if the coefficients are doubled. Since n appears in the denominator in the Nernst equation, this will affect the value of E.
- Q: The reaction quotient (Q) will be squared since the concentrations of the reactants and products are to the power of their stoichiometric coefficients in the expression for Q.
Therefore, the effects on the quantities are as follows: InQ is squared, Eo has no change, E is affected by the change in n and therefore indirectly by the change in coefficients, n is doubled, and Q is squared.