Consider a cell consisting of Zn(s)|Zn²⁺ (1.00×10^-5 M)|| Ag⁺(0.10M)|Ag(s) and standard reduction potentials of the cell are E°_Zn(red)=-0.76V and E°_Ag(red)=0.80V at 25°C. For this cell the following parameters age given

The cell reaction is

i. Zn(s)+2Ag⁺(aq)=> Zn²⁺(aq)+2Ag(s)

ii.E_cell=1.6488V

iii.ΔG°=-3.01×10⁵J

Which of the following is more appropriate? 

এখানে,

zn-অ্যানোড

Ag-ক্যাথোড

i. $\mathrm{Zn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$

ii.

$\begin{aligned} E_{\text {cell }}^{0} & =E_{\text {Zn(ox) }}^{0}+E_{\text {Ag(red) }}^{0} \\ & =+0.76+0.80 \\ & =1.56 \mathrm{~V}\end{aligned}$

$E = E^\circ - \frac{RT}{nF} \ln Q.$ ২৫°C-এ $\frac{RT}{F} \approx 0.025692 \text{ V}$

$E = 1.56 - \frac{0.025692}{2} \ln(1 \times 10^{-3}) = 1.56 - 0.012846(-6.9078) = 1.6488 \text{ V.}$

iii.

$\begin{aligned} \Delta G^{0} & =-n F E_{\text {cell }}^{0} \\ & =-2 \times 96500 \times 1.56 \\ & =-3.01 \times 10^{5} \mathrm{~J}\end{aligned}$

অতএব – i, ii ও iii সবগুলোই উপযুক্ত এবং সঠিক।