Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (c) Oxidation of Ag(s) by Pb²⁺(aq)

검증된 단계별 안내

Identify the half-reactions involved in the oxidation of Ag(s) by Pb^{2+}(aq).

Write the reduction half-reaction for Pb^{2+}(aq) to Pb(s) and the oxidation half-reaction for Ag(s) to Ag^{+}(aq).

Look up the standard reduction potentials (E^0) for each half-reaction from Appendix D.

Calculate the standard cell potential (E^0_{cell}) by subtracting the standard reduction potential of the oxidation half-reaction from the standard reduction potential of the reduction half-reaction.

Determine if the reaction is spontaneous under standard-state conditions by checking if the calculated E^0_{cell} is positive.

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Standard-State Conditions

Standard-state conditions refer to a set of specific conditions used to measure the properties of substances. These conditions typically include a temperature of 25°C (298 K), a pressure of 1 atm, and concentrations of 1 M for solutions. Understanding these conditions is crucial for predicting the feasibility of chemical reactions, as they provide a baseline for comparing thermodynamic data.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Identifying the oxidizing and reducing agents is essential for predicting whether a reaction can occur, particularly in the context of standard electrode potentials.

Electrode Potentials and Gibbs Free Energy

Electrode potentials, measured in volts, indicate the tendency of a species to gain or lose electrons in a redox reaction. The standard electrode potential (E°) can be used to calculate the Gibbs free energy change (ΔG°) for a reaction using the equation ΔG° = -nFE°, where n is the number of moles of electrons transferred and F is Faraday's constant. A negative ΔG° indicates that a reaction is spontaneous under standard-state conditions.

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (c) Oxidation of Ag(s) by Pb2+(aq)