329961 If the pressure of \({{\rm{H}}_{\rm{2}}}\) gas is increased from 1 atm to 100 atm, keeping \({{\rm{H}}^{\rm{ + }}}\) concentration constant at 1 M, the oxidation potential of hydrogen half cell at \({\rm{25^\circ C}}\) will be

329962 In the electrochemical cell :-
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{(1}}{\rm{.0M)}}} \right \vert {\rm{Cu}}\), the emf of this Daniel cell is \({{\rm{E}}_{\rm{1}}}\). When the concentration of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}\) is changed to 1.0 M and that of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) changed to 0.01 M, the emf changes to \({{\rm{E}}_{\rm{2}}}\). From the following, which one is the relationship between \({{\rm{E}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{E}}_{\rm{2}}}\) ? \({\rm{(Given}}\,\,\frac{{{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059)}}\)

329963 Given \({\rm{E}}_{{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.72 V,E}}_{{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.42 V}}\)
The potential for the cell
\(\left. {{\rm{Cr}}} \right \vert \left. {{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{(0}}{\rm{.1M)}}} \right\vert \left. {{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{(0}}{\rm{.01 M)}}} \right \vert {\rm{Fe}}\) is

329964 Which one of the following will increase the voltage of the cell with the following cell reaction?
\(Sn + 2A{g^ + } \to S{n^{2 + }} + 2Ag\)

329961 If the pressure of \({{\rm{H}}_{\rm{2}}}\) gas is increased from 1 atm to 100 atm, keeping \({{\rm{H}}^{\rm{ + }}}\) concentration constant at 1 M, the oxidation potential of hydrogen half cell at \({\rm{25^\circ C}}\) will be

329962 In the electrochemical cell :-
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{(1}}{\rm{.0M)}}} \right \vert {\rm{Cu}}\), the emf of this Daniel cell is \({{\rm{E}}_{\rm{1}}}\). When the concentration of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}\) is changed to 1.0 M and that of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) changed to 0.01 M, the emf changes to \({{\rm{E}}_{\rm{2}}}\). From the following, which one is the relationship between \({{\rm{E}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{E}}_{\rm{2}}}\) ? \({\rm{(Given}}\,\,\frac{{{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059)}}\)

329963 Given \({\rm{E}}_{{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.72 V,E}}_{{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.42 V}}\)
The potential for the cell
\(\left. {{\rm{Cr}}} \right \vert \left. {{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{(0}}{\rm{.1M)}}} \right\vert \left. {{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{(0}}{\rm{.01 M)}}} \right \vert {\rm{Fe}}\) is

329964 Which one of the following will increase the voltage of the cell with the following cell reaction?
\(Sn + 2A{g^ + } \to S{n^{2 + }} + 2Ag\)

329961 If the pressure of \({{\rm{H}}_{\rm{2}}}\) gas is increased from 1 atm to 100 atm, keeping \({{\rm{H}}^{\rm{ + }}}\) concentration constant at 1 M, the oxidation potential of hydrogen half cell at \({\rm{25^\circ C}}\) will be

329962 In the electrochemical cell :-
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{(1}}{\rm{.0M)}}} \right \vert {\rm{Cu}}\), the emf of this Daniel cell is \({{\rm{E}}_{\rm{1}}}\). When the concentration of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}\) is changed to 1.0 M and that of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) changed to 0.01 M, the emf changes to \({{\rm{E}}_{\rm{2}}}\). From the following, which one is the relationship between \({{\rm{E}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{E}}_{\rm{2}}}\) ? \({\rm{(Given}}\,\,\frac{{{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059)}}\)

329963 Given \({\rm{E}}_{{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.72 V,E}}_{{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.42 V}}\)
The potential for the cell
\(\left. {{\rm{Cr}}} \right \vert \left. {{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{(0}}{\rm{.1M)}}} \right\vert \left. {{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{(0}}{\rm{.01 M)}}} \right \vert {\rm{Fe}}\) is

329964 Which one of the following will increase the voltage of the cell with the following cell reaction?
\(Sn + 2A{g^ + } \to S{n^{2 + }} + 2Ag\)

329961 If the pressure of \({{\rm{H}}_{\rm{2}}}\) gas is increased from 1 atm to 100 atm, keeping \({{\rm{H}}^{\rm{ + }}}\) concentration constant at 1 M, the oxidation potential of hydrogen half cell at \({\rm{25^\circ C}}\) will be

329962 In the electrochemical cell :-
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{ZnS}}{{\rm{O}}_{\rm{4}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{(1}}{\rm{.0M)}}} \right \vert {\rm{Cu}}\), the emf of this Daniel cell is \({{\rm{E}}_{\rm{1}}}\). When the concentration of \({\rm{ZnS}}{{\rm{O}}_{\rm{4}}}\) is changed to 1.0 M and that of \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}\) changed to 0.01 M, the emf changes to \({{\rm{E}}_{\rm{2}}}\). From the following, which one is the relationship between \({{\rm{E}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{E}}_{\rm{2}}}\) ? \({\rm{(Given}}\,\,\frac{{{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059)}}\)

329963 Given \({\rm{E}}_{{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.72 V,E}}_{{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.42 V}}\)
The potential for the cell
\(\left. {{\rm{Cr}}} \right \vert \left. {{\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{(0}}{\rm{.1M)}}} \right\vert \left. {{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{(0}}{\rm{.01 M)}}} \right \vert {\rm{Fe}}\) is

329964 Which one of the following will increase the voltage of the cell with the following cell reaction?
\(Sn + 2A{g^ + } \to S{n^{2 + }} + 2Ag\)