What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ concentration is 0.0120 M and the Ag⁺ concentration is 1.25 M? A) 9.60 $\times$ 10^-3 B) 7.68 $\times$ 10^-3 C) 104 D) 1.25 $\times$ 10^-2 E) 130

Question

Quizplus · Accepted Answer

The voltaic cell is composed of a zinc half-cell, ZnS1U1P12+ → Zn2+ + 2e−, and a silver half-cell, Ag+ + e− → AgS1U1P1.

To find the reaction quotient, Q, we need to write the balanced overall reaction for the cell and calculate the concentrations of the species involved:

ZnS1U1P12+ + Ag+ → Zn2+ + AgS1U1P1

At equilibrium, Q = [Zn2+][AgS1U1P1] / [ZnS1U1P12+][Ag+]

Plugging in the given concentrations:

Q = (1.25 M) / (0.0120 M) = 104

Therefore, the best choice is B, 7.68 x 10^10.

What Is the Value of the Reaction Quotient,Q,for the Voltaic ×\times×

What Is the Value of the Reaction Quotient,Q,for the Voltaic $\times$