Question

Consider the following reaction in a galvanic cell: \[ \mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu} \] What is the Gibb's free energy in kJ/ mol for the reaction under standard conditions? 212.3 \( -212.3 \) 106.15 \( -106.15 \)

          Consider the following reaction in a galvanic cell:
\[
\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}
\]

What is the Gibb's free energy in kJ/ mol for the reaction under standard conditions?
212.3
\( -212.3 \)
106.15
\( -106.15 \)

Consider the following reaction in a galvanic cell:

Zn+Cu^2+→Zn^2++Cu

What is the Gibb's free energy in kJ/ mol for the reaction under standard conditions?
212.3
-212.3
106.15
-106.15

Added by Julian H.

Chemistry: The Molecular Science

John W. Moore, Conrad L. Stanitski,… 3rd Edition

Chapter 19

Instant Answer

Solved by Expert Lijeesh Krishnan

Step 1

The Gibbs Free Energy (\( \Delta G \)) of a reaction can be calculated using the equation: \[ \Delta G = -nFE \] where \( n \) is the number of moles of electrons transferred in the reaction, \( F \) is the Faraday constant (approximately \( 96,485 \, C/mol \) of Show more…

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Consider the following reaction in a galvanic cell: \[ \mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu} \] What is the Gibb's free energy in kJ/ mol for the reaction under standard conditions? 212.3 \( -212.3 \) 106.15 \( -106.15 \)