The standard electrode potential -E-circ- Daniel cell is -1-1 V- Calculate Delta G-circ- the reaction-Zn-s- - Cu-aq-2- rightarrow Zn-aq-2- - Cu-s-1 F - 96500 C-mol-

Question

Toppr Admin · Accepted Answer

-x394-G-x2212-nFE-x2212-2-xD7-96500-xD7-2-2-xA0-x2212-212300-xA0-J-x2212-212-3-xA0-kJ

The standard electrode potential $(E^{\circ})$ for Daniel cell is $+ 1.1 V$ . Calculate $Δ G^{\circ}$ for the reaction.
$Z n (s) + C u_{(a q)}^{2 +} \to Z n_{(a q)}^{2 +} + C u (s)$
$(1 F = 96500 C / m o l)$

$Δ G = - n F E$
$= - 2 \times 96500 \times 2.2$
= $- 212300 J$
= $- 212.3 k J$

The standard electrode potential (E∘) for Daniel cell is +1.1 V. Calculate ΔG∘ for the reaction.Zn(s)+Cu2+(aq)→Zn2+(aq)+Cu(s)(1 F=96500 C/mol)

ΔG=−nFE=−2×96500×2.2 =−212300 J=−212.3 kJ

The standard electrode potential $(E^{\circ})$ for Daniel cell is $+ 1.1 V$ . Calculate $Δ G^{\circ}$ for the reaction.
$Z n (s) + C u_{(a q)}^{2 +} \to Z n_{(a q)}^{2 +} + C u (s)$
$(1 F = 96500 C / m o l)$

$Δ G = - n F E$
$= - 2 \times 96500 \times 2.2$
= $- 212300 J$
= $- 212.3 k J$