Calculate the standard free-energy change at 25^∘ C for the following reaction. 3 Cu(s)+2 NO3^-(

step 1 So here we're given a specific reaction. We have copper metal reacting with the nitrate ion, ani

Calculate the standard free-energy change at 25^∘ C for the...

Calculate the standard free-energy change at $25^{\circ} \mathrm{C}$ for the following reaction. $3 \mathrm{Cu}(s)+2 \mathrm{NO}_{3}^{-}(a q)+8 \mathrm{H}^{+}(a q) \longrightarrow$ $$3 \mathrm{Cu}^{2+}(a q)+2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)$$ Use standard electrode potentials.

Calculate the standard free-energy change at $25^{\circ} \mathrm{C}$ for the following reaction.
$3 \mathrm{Cu}(s)+2 \mathrm{NO}_{3}^{-}(a q)+8 \mathrm{H}^{+}(a q) \longrightarrow$
$$3 \mathrm{Cu}^{2+}(a q)+2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)$$
Use standard electrode potentials.

Key Concepts

Half-Reactions

Half-reactions represent the individual oxidation and reduction processes that occur at the electrodes in a redox reaction. They are used to break down complex redox reactions into simpler parts, facilitating the balancing of the overall reaction and the determination of the number of electrons transferred.

Electron Transfer Number (n)

The number of electrons transferred in an electrochemical reaction, denoted as n, is crucial for calculating the overall free energy change and cell potential. It accounts for the stoichiometry of the reaction and is used in the equation ?G° = -nFE° to convert the electrical energy per mole of electrons into thermodynamic energy.

Standard Electrode Potentials

Standard electrode potentials are quantitative measures of the tendency of a chemical species to be reduced, measured under standard conditions relative to the standard hydrogen electrode. They are used to predict the direction of redox reactions and to calculate the electromotive force (EMF) of an electrochemical cell by comparing the potentials of the cathode and anode half?reactions.

Gibbs Free Energy Change

The Gibbs free energy change (?G°) indicates the spontaneity of a reaction under standard conditions, with a negative ?G° signifying a spontaneous process. For electrochemical reactions, it is directly related to the cell potential through the equation ?G° = -nFE°, linking thermodynamic favorability with electrical potential.

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