If Cu^{+} + e^- to Cu ; E^o = X_1 and Cu^{2+} | vedclass

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

Question

(A) The standard Gibbs free energy change is given by $\Delta G^o = -nFE^o$.For the reaction $Cu^{2+} + 2e^- 	o Cu$,$\Delta G_1^o = -2FX_2$.For the r

Vedclass · Accepted Answer

$2X_2 - X_1$

Vedclass · Answer

(A) The standard Gibbs free energy change is given by $\Delta G^o = -nFE^o$.For the reaction $Cu^{2+} + 2e^- 	o Cu$,$\Delta G_1^o = -2FX_2$.For the reaction $Cu^{+} + e^- 	o Cu$,$\Delta G_2^o = -FX_1$.We want to find $E^o$ for $Cu^{2+} + e^- 	o Cu^{+}$. This reaction can be obtained by subtracting the second reaction from the first:$(Cu^{2+} + 2e^- 	o Cu) - (Cu^{+} + e^- 	o Cu) \implies Cu^{2+} + e^- 	o Cu^{+}$.Therefore,$\Delta G_3^o = \Delta G_1^o - \Delta G_2^o$.$-FE^o = -2FX_2 - (-FX_1)$.$-FE^o = -2FX_2 + FX_1$.Dividing by $-F$,we get $E^o = 2X_2 - X_1$.

If $Cu^{+} + e^- \to Cu$ ; $E^o = X_1$ and $Cu^{2+} + 2e^- \to Cu$ ; $E^o = X_2$,then the value of $E^o$ for $Cu^{2+} + e^- \to Cu^{+}$ will be

Similar Questions

Give the symbolic representation of the following half-cells (electrodes):
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$

The tendency of an electrode to lose electrons is known as

Which of the following metals cannot displace $H_2$ from acids or $H_2O$ from its compounds?

If $Cu^{2+} + 2e^{-} \rightarrow Cu, E^{0} = 0.337 \ V$ and $Cu^{2+} + e^{-} \rightarrow Cu^{+}, E^{0} = 0.153 \ V$,then for the reaction $Cu^{+} + e^{-} \rightarrow Cu$,$E^{0}_{cell} =$ .............. $V$.

Given:
$E^o_{Cr^{3+}/Cr} = -0.74 \ V$,$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V$,$E^o_{Cl_2/Cl^{-}} = 1.36 \ V$
Based on the data given above,the strongest oxidising agent will be:

Vedclass Test Series

Exam Paper Generator

Online Exam Module