For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25° C. The value of standard Gibbs energy, Δ G° will be (F=96500 C mol -1)

Question

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25° C. The value of standard Gibbs energy, Δ G° will be (F=96500 C mol -1) (A) - 89.0 kJ (B) - 89.0 J (C) - 44.5 kJ (D) - 98.0 kJ

Tardigrade Admin · Accepted Answer

We know that, standard Gibbs energy, Δ G0=-n F E text cell 0 For the cell reaction, 2 A g++C u arrow C u2++2 A g Δ Ec e l l0=+0.46 V Δ G0=-n F Ec e l l0 n =2 Δ G0=-2 × 96500 × 0.46 =-88780 J =-88.7 kJ ≈-89.0 kJ

Q. For the reduction of silver ions with copper metal, the standard cell potential was found to be $+ 0.46 V$ at $2 5^{\circ} C$ . The value of standard Gibbs energy, $Δ G^{\circ}$ will be
$(F = 96500 C m o l^{- 1})$

- 89.0 kJ

- 89.0 J

- 44.5 kJ

- 98.0 kJ

We know that, standard Gibbs energy,
$Δ G^{0} = - n F E_{cell}^{0}$
For the cell reaction,
$2 A g^{+} + C u \to C u^{2 +} + 2 A g$
$Δ E_{ce ll}^{0} = + 0.46 V$
$Δ G^{0} = - n F E_{ce ll}^{0}$
$n = 2$
$Δ G^{0} = - 2 \times 96500 \times 0.46$
$= - 88780 J$
$= - 88.7 k J \approx - 89.0 k J$

Q. For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46V at 25∘C. The value of standard Gibbs energy, ΔG∘ will be (F=96500Cmol−1)