The standard electrode potential for Daniell cell is 1.1 volt. What is the standard Gibbs energy for the reaction?

Question

The standard electrode potential for Daniell cell is 1.1 volt. What is the standard Gibbs energy for the reaction? (A)  212.3 kJ mol-1 (B)  - 212.3 kJ mol-1 (C) 106.15 kJ mol-1 (D)  -106.15 kJ mol-1

Tardigrade Admin · Accepted Answer

Net reaction occurring in a Daniell cell is Zn(s) + Cu2+(aq) arrow Zn2+(aq) + Cu(s) Δ = - nFE° = -2 × 69500 × 1.1 = -212300 J mol-1 = 212.3 kJ mol-1

Q. The standard electrode potential for Daniell cell is $1.1 v o lt$ . What is the standard Gibbs energy for the reaction?

$212.3 k J m o l^{- 1}$

$- 212.3 k J m o l^{- 1}$

$106.15 k J m o l^{- 1}$

$- 106.15 k J m o l^{- 1}$

Net reaction occurring in a Daniell cell is
$Z n_{(s)} + C u_{(a q)}^{2 +} \to Z n_{(a q)}^{2 +} + C u_{(s)}$
$Δ = - n F E^{\circ} = - 2 \times 69500 \times 1.1$
$= - 212300 J m o l^{- 1} = 212.3 k J m o l^{- 1}$

Q. The standard electrode potential for Daniell cell is 1.1volt. What is the standard Gibbs energy for the reaction?

212.3kJmol−1

−212.3kJmol−1

106.15kJmol−1

−106.15kJmol−1