For the cell,Mn_{(s)} | Mn^{2+}_{(aq)} (0.4 , | vedclass

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

Question

(B) The cell reaction is: $Mn_{(s)} + Sn^{2+}_{(aq)} \rightarrow Mn^{2+}_{(aq)} + Sn_{(s)}$.Standard cell potential $E^o_{cell} = E^o_{cathode} - E^o_

Vedclass · Accepted Answer

$-194.93$

Vedclass · Answer

(B) The cell reaction is: $Mn_{(s)} + Sn^{2+}_{(aq)} ightarrow Mn^{2+}_{(aq)} + Sn_{(s)}$.Standard cell potential $E^o_{cell} = E^o_{cathode} - E^o_{anode} = E^o_{Sn^{2+}/Sn} - E^o_{Mn^{2+}/Mn} = -0.14 - (-1.18) = 1.04 \, V$.The Nernst equation at $298 \, K$ is: $E_{cell} = E^o_{cell} - \frac{0.06}{n} \log \frac{[Mn^{2+}]}{[Sn^{2+}]}$.Here $n = 2$,$[Mn^{2+}] = 0.4$,and $[Sn^{2+}] = 0.04$.$E_{cell} = 1.04 - \frac{0.06}{2} \log \frac{0.4}{0.04} = 1.04 - 0.03 \log(10) = 1.04 - 0.03 = 1.01 \, V$.Free energy change $\Delta G = -nFE_{cell} = -2 	imes 96500 	imes 1.01 \, J = -194930 \, J = -194.93 \, kJ$.

For the cell,$Mn_{(s)} | Mn^{2+}_{(aq)} (0.4 \, M) || Sn^{2+}_{(aq)} (0.04 \, M) | Sn_{(s)}$,calculate the free energy change $(\Delta G)$ at $298 \, K$ in $kJ$. Given: $E^o_{Mn^{2+}/Mn} = -1.18 \, V$; $E^o_{Sn^{2+}/Sn} = -0.14 \, V$; $\frac{2.303RT}{F} = 0.06$.

Similar Questions

When a copper plate is kept in a $0.1 \ M$ solution of $CuSO_4$ at $298 \ K$ temperature and if $70 \ \%$ dissociation has occurred,then calculate the potential of the copper electrode.

Calculate $E_{cell}$ of the reaction in $V$:
$Mg_{(s)} + 2Ag^{+}(0.0001 \ M) \to Mg^{+2}(0.100 \ M) + 2Ag_{(s)}$
Given that $E_{cell}^o = 3.17 \ V$.

If $A$ is the reactant and $P$ is the product,which one of the following is the correct form of the Nernst equation?

The standard cell potential of a cell reaction involving the transfer of $2$ electrons at $25^{\circ}C$ is $0.295 \ V$. What is its equilibrium constant at $25^{\circ}C$?

Fill in the blanks :
$1.$ The ratio of concentration of products to concentration of reactants is ........
$2.$ $\ln(\log(x)) =$ ............
$3.$ At equilibrium,between $E_{cell}$ and $E_{cell}^{o}$,......... will be zero.

Vedclass Test Series

Exam Paper Generator

Online Exam Module