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Question

Chemistry Question on Gibbs Free Energy

The standard electrode potential for Daniell cell is 1.1 volt1.1\, volt. What is the standard Gibbs energy for the reaction?

A

\ce212.3 kJ mol−1\ce{ 212.3 \, kJ \, mol^{-1}}

B

\ce−212.3 kJ mol−1\ce{ - 212.3 \, kJ \, mol^{-1}}

C

\ce106.15 kJ mol−1\ce{106.15 \, kJ \, mol^{-1}}

D

\ce−106.15 kJ mol−1\ce{ -106.15 \, kJ \, mol^{-1}}

Answer

\ce−212.3 kJ mol−1\ce{ - 212.3 \, kJ \, mol^{-1}}

Explanation

Solution

Net reaction occurring in a Daniell cell is Zn(s)+Cu(aq)2+−>Zn(aq)2++Cu(s) { Zn_{(s)} + Cu^{2+}_{(aq)} - > Zn^{2+}_{(aq)} + Cu_{(s)}} Δ=−nFE∘=−2×69500×1.1\Delta = - nFE^\circ = -2 \times 69500 \times 1.1 =−212300 J mol−1=212.3 kJ mol−1 {= -212300 \, J \, mol^{-1} = 212.3 \, kJ \, mol^{-1} }