The cell reaction of an electrochemical cell is \(Cu^{2+}(C_{1}) + Zn \to Cu + Zn^{2+}(C_{2})\).

The change in free energy will be the function of:

\(1. \ ln (C_{1}+C_{2})\)
2. \(ln (\frac{C_{2}}{C_{1}})\)
\(3. \ ln C_{2}\)
\(4. \ lnC_{1}\)

A cell reaction become spontaneous when:

1. ∆Gº is negative

2. ∆Gº is positive

3. $E_{Red}^{°}$ is positive

4. $E_{Red}^{°}$ is negative

The standard Emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25 ºC. The equilibrium constant of the reaction would be:

(Given F = 96500 C mol^–1; R = 8.314 J K^–1 mol^–1) 

1. 4.0 × 10¹²

2. 1.0 × 10²

3. 1.0 × 10¹⁰

4. 2.0 × 10¹¹