330411 The minimum voltage required to electrolyse alumina in the Hall - Heroult process is
\(\left( {{\rm{ Given, \Delta G}}_{\rm{f}}^{\rm{0}}\left( {{\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}} \right){\rm{ = - 1520 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right.{\rm{;}}\)
\(\left. {{\rm{\Delta G}}_{\rm{f}}^{\rm{o}}\left( {{\rm{C}}{{\rm{O}}_{\rm{2}}}} \right){\rm{ = - 394 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right)\)

330412 Assertion :
A reaction is spontaneous if \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}\).
Reason :
For \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}, \Delta \mathrm{G}\) is always \(-\mathrm{ve}\).

330413 Assertion :
An electrochemical cell can be set up only if the redox reaction is spontaneous.
Reason :
A reaction is spontaneous if standard free energy change is negative.

330414 Given the standard potential of the following at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{3 + }};{\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{0}}.{\rm{95}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{M}}{{\rm{n}}^{3 + }} \to {\rm{M}}{{\rm{n}}^{2 + }};\quad {\mkern 1mu} \,\,{\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{1}}.{\rm{51}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{The}}{\mkern 1mu} \,\,{\rm{standard}}\,\,{\mkern 1mu} {\rm{potential}}\,{\rm{of}}{\mkern 1mu} \)
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{2 + }}{\rm{ is }}\)

330415 The Gibbs energy for the decomposition of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is as follows
\(\frac{2}{3}A{l_2}{O_3} \to \frac{4}{3}Al + {O_2}{\Delta _r}G = + 966 kJ\,\,mo{l^{ - 1}}\)
The potential difference needed for electrolytic reduction of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is at least

330411 The minimum voltage required to electrolyse alumina in the Hall - Heroult process is
\(\left( {{\rm{ Given, \Delta G}}_{\rm{f}}^{\rm{0}}\left( {{\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}} \right){\rm{ = - 1520 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right.{\rm{;}}\)
\(\left. {{\rm{\Delta G}}_{\rm{f}}^{\rm{o}}\left( {{\rm{C}}{{\rm{O}}_{\rm{2}}}} \right){\rm{ = - 394 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right)\)

330412 Assertion :
A reaction is spontaneous if \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}\).
Reason :
For \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}, \Delta \mathrm{G}\) is always \(-\mathrm{ve}\).

330413 Assertion :
An electrochemical cell can be set up only if the redox reaction is spontaneous.
Reason :
A reaction is spontaneous if standard free energy change is negative.

330414 Given the standard potential of the following at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{3 + }};{\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{0}}.{\rm{95}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{M}}{{\rm{n}}^{3 + }} \to {\rm{M}}{{\rm{n}}^{2 + }};\quad {\mkern 1mu} \,\,{\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{1}}.{\rm{51}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{The}}{\mkern 1mu} \,\,{\rm{standard}}\,\,{\mkern 1mu} {\rm{potential}}\,{\rm{of}}{\mkern 1mu} \)
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{2 + }}{\rm{ is }}\)

330415 The Gibbs energy for the decomposition of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is as follows
\(\frac{2}{3}A{l_2}{O_3} \to \frac{4}{3}Al + {O_2}{\Delta _r}G = + 966 kJ\,\,mo{l^{ - 1}}\)
The potential difference needed for electrolytic reduction of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is at least

330411 The minimum voltage required to electrolyse alumina in the Hall - Heroult process is
\(\left( {{\rm{ Given, \Delta G}}_{\rm{f}}^{\rm{0}}\left( {{\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}} \right){\rm{ = - 1520 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right.{\rm{;}}\)
\(\left. {{\rm{\Delta G}}_{\rm{f}}^{\rm{o}}\left( {{\rm{C}}{{\rm{O}}_{\rm{2}}}} \right){\rm{ = - 394 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right)\)

330412 Assertion :
A reaction is spontaneous if \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}\).
Reason :
For \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}, \Delta \mathrm{G}\) is always \(-\mathrm{ve}\).

330413 Assertion :
An electrochemical cell can be set up only if the redox reaction is spontaneous.
Reason :
A reaction is spontaneous if standard free energy change is negative.

330414 Given the standard potential of the following at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{3 + }};{\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{0}}.{\rm{95}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{M}}{{\rm{n}}^{3 + }} \to {\rm{M}}{{\rm{n}}^{2 + }};\quad {\mkern 1mu} \,\,{\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{1}}.{\rm{51}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{The}}{\mkern 1mu} \,\,{\rm{standard}}\,\,{\mkern 1mu} {\rm{potential}}\,{\rm{of}}{\mkern 1mu} \)
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{2 + }}{\rm{ is }}\)

330415 The Gibbs energy for the decomposition of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is as follows
\(\frac{2}{3}A{l_2}{O_3} \to \frac{4}{3}Al + {O_2}{\Delta _r}G = + 966 kJ\,\,mo{l^{ - 1}}\)
The potential difference needed for electrolytic reduction of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is at least

330411 The minimum voltage required to electrolyse alumina in the Hall - Heroult process is
\(\left( {{\rm{ Given, \Delta G}}_{\rm{f}}^{\rm{0}}\left( {{\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}} \right){\rm{ = - 1520 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right.{\rm{;}}\)
\(\left. {{\rm{\Delta G}}_{\rm{f}}^{\rm{o}}\left( {{\rm{C}}{{\rm{O}}_{\rm{2}}}} \right){\rm{ = - 394 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right)\)

330412 Assertion :
A reaction is spontaneous if \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}\).
Reason :
For \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}, \Delta \mathrm{G}\) is always \(-\mathrm{ve}\).

330413 Assertion :
An electrochemical cell can be set up only if the redox reaction is spontaneous.
Reason :
A reaction is spontaneous if standard free energy change is negative.

330414 Given the standard potential of the following at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{3 + }};{\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{0}}.{\rm{95}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{M}}{{\rm{n}}^{3 + }} \to {\rm{M}}{{\rm{n}}^{2 + }};\quad {\mkern 1mu} \,\,{\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{1}}.{\rm{51}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{The}}{\mkern 1mu} \,\,{\rm{standard}}\,\,{\mkern 1mu} {\rm{potential}}\,{\rm{of}}{\mkern 1mu} \)
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{2 + }}{\rm{ is }}\)

330415 The Gibbs energy for the decomposition of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is as follows
\(\frac{2}{3}A{l_2}{O_3} \to \frac{4}{3}Al + {O_2}{\Delta _r}G = + 966 kJ\,\,mo{l^{ - 1}}\)
The potential difference needed for electrolytic reduction of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is at least

330411 The minimum voltage required to electrolyse alumina in the Hall - Heroult process is
\(\left( {{\rm{ Given, \Delta G}}_{\rm{f}}^{\rm{0}}\left( {{\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}} \right){\rm{ = - 1520 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right.{\rm{;}}\)
\(\left. {{\rm{\Delta G}}_{\rm{f}}^{\rm{o}}\left( {{\rm{C}}{{\rm{O}}_{\rm{2}}}} \right){\rm{ = - 394 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}} \right)\)

330412 Assertion :
A reaction is spontaneous if \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}\).
Reason :
For \(\mathrm{E}_{\text {cell }}=+\mathrm{ve}, \Delta \mathrm{G}\) is always \(-\mathrm{ve}\).

330413 Assertion :
An electrochemical cell can be set up only if the redox reaction is spontaneous.
Reason :
A reaction is spontaneous if standard free energy change is negative.

330414 Given the standard potential of the following at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{3 + }};{\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{0}}.{\rm{95}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{M}}{{\rm{n}}^{3 + }} \to {\rm{M}}{{\rm{n}}^{2 + }};\quad {\mkern 1mu} \,\,{\mkern 1mu} {{\rm{E}}^ \ominus } = {\rm{1}}.{\rm{51}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\)
\({\rm{The}}{\mkern 1mu} \,\,{\rm{standard}}\,\,{\mkern 1mu} {\rm{potential}}\,{\rm{of}}{\mkern 1mu} \)
\({\rm{Mn}}{{\rm{O}}_2} \to {\rm{M}}{{\rm{n}}^{2 + }}{\rm{ is }}\)

330415 The Gibbs energy for the decomposition of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is as follows
\(\frac{2}{3}A{l_2}{O_3} \to \frac{4}{3}Al + {O_2}{\Delta _r}G = + 966 kJ\,\,mo{l^{ - 1}}\)
The potential difference needed for electrolytic reduction of \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\,\,{\rm{at}}\,\,{\rm{500^\circ C}}\) is at least