(a) In the Nernst equation, what is the numerical value of the reaction quotient, Q, under standard conditions? (b) Can the Nernst equation be used at temperatures other than room temperature?

Before we can find the numerical value of Q, we first need to review the Nernst equation, which is given by: \(E = E^0 - \frac{RT}{nF} \ln Q\) where: - \(E\) is the cell potential at any point in time, - \(E^0\) is the standard electrode potential, - \(R\) is the gas constant, - \(T\) is the temperature in Kelvin, - \(n\) is the number of electrons transferred in the redox reaction, - \(F\) is Faraday's constant, and - \(Q\) is the reaction quotient. Under standard conditions, the cell potential (\(E\)) is equal to the standard electrode potential (\(E^0\)) because the reaction is at equilibrium. As a result, the reactant and product activities are at their standard states, so the reaction quotient, Q, equals 1. Therefore, the numerical value of Q under standard conditions is 1.

The Nernst equation is a general equation that relates the cell potential to the temperature, reaction quotient, and number of electrons transferred in a half-cell reaction. This means that the equation is not limited to a specific temperature, such as room temperature. In fact, one of the main uses of the Nernst equation is to be able to calculate the potential of an electrochemical cell under different temperatures and concentrations. The equation inherently includes temperature as one of its parameters, which means it can be applied to different temperatures as long as you adjust the value of T (temperature in Kelvin) accordingly.