The standard cell potential (E°_cell)for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of [Cu²⁺] = 1.0 × 10^-5 M and [Zn²⁺] = 3.5 M. Zn (s)+ Cu²⁺ (aq)→ Cu (s)+ Zn²⁺ (aq) A)1.42 B)1.26 C)0.94 D)0.78 E)1.10

Question

Quizplus · Accepted Answer

The cell potential can be calculated using the Nernst equation:
Ecell = E°cell - (RT/nF)ln(Q)
where R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the balanced equation, F is Faraday's constant, Q is the reaction quotient.
Firstly, calculate the value of Q
Q = ([Cu2+]/[Zn2+]) = ([1.0 × 10^-5]/[3.5]) = 2.86 × 10^-6
Next, substitute the given values:
Ecell = +1.10 - (0.0257/2)ln(2.86 × 10^-6)
Ecell = 0.94 V
Therefore, the best choice is C.

The Standard Cell Potential (E°cell)for the Reaction Below Is +1

The Standard Cell Potential (E°_cell)for the Reaction Below Is +1