The standard Gibbs free energy change (Delta | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The reaction in a $Daniell$ cell is: $Zn_{(s)} + Cu^{2+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$.For $1 \, mole$ of $Zn$ oxidation,$n = 2$ e

Vedclass · Accepted Answer

$-424.6$

Vedclass · Answer

(C) The reaction in a $Daniell$ cell is: $Zn_{(s)} + Cu^{2+}_{(aq)} ightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$.For $1 \, mole$ of $Zn$ oxidation,$n = 2$ electrons are transferred.For $2 \, moles$ of $Zn$ oxidation,the number of electrons transferred is $n = 2 	imes 2 = 4$.Given $E^{\circ}_{cell} = 1.1 \, V$ and $F = 96500 \, C \, mol^{-1}$.The formula for standard Gibbs free energy change is $\Delta G^{\circ} = -n F E^{\circ}_{cell}$.Substituting the values: $\Delta G^{\circ} = -4 	imes 96500 \, C \, mol^{-1} 	imes 1.1 \, V$.$\Delta G^{\circ} = -424600 \, J \, mol^{-1} = -424.6 \, kJ \, mol^{-1}$.

The standard Gibbs free energy change ($\Delta G^{\circ}$ in $kJ \, mol^{-1}$),in a $Daniell$ cell $(E^{\circ}_{cell} = 1.1 \, V)$,when $2 \, moles$ of $Zn_{(s)}$ is oxidised at $298 \, K$,is closest to

Similar Questions

What is an electrode and a half-cell? Explain their symbolic representation with a suitable example.

Which one of the following statements is true for a standard electrochemical cell involving $H_2$ and $Cu$ electrodes?

The electrochemical cell is set up as follows: $Pt (H_2, 1 \, atm) | HCl (0.1 \, M) || \text{Acetic Acid} (0.1 \, M) | (H_2, 1 \, atm) Pt$. The $E.M.F.$ of the cell is not zero because:

Fill in the blanks :
$1.$ $E_{cell}^o$ of Daniell cell $= $ ........... .
$2.$ In Daniell cell,$n = $ ........... .
$3.$ For $Al + 3Ag^{+} \rightarrow Al^{3+} + 3Ag,$ $n = $ ...........

Which of the following statements is incorrect during the discharge of a lead storage battery?

Vedclass Test Series

Exam Paper Generator

Online Exam Module