What is $\varepsilon$ $\circ$ _cell for the following electrochemical equation? ($\varepsilon$ $\circ$ _red(Li⁺/Li)= -3.04 V$\varepsilon$ $\circ$ _red(Cu²⁺/Cu)= 0.342 V) 2Li(s)+ Cu²⁺(aq)$\to$ 2Li⁺(aq)+ Cu(s)

Question

Quizplus · Accepted Answer

First, we need to calculate the standard potential (E°) for the given equation using the given standard reduction potentials:
E° = E°(Li+) - E°(Cu2+) = (-3.04 V) - (0.342 V) = -3.382 V
Then, we plug in the calculated E° in the Nernst equation:
E = E° - (RT/nF)lnQ
where R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred, F is the Faraday constant, and Q is the reaction quotient.
Since the reaction is at standard conditions, Q = 1 and lnQ = 0, so the equation simplifies to:
E = E°
Therefore, the final answer is -3.382 V.

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