Relation between Gibbs free energy, Equilibrium constant and emf of cell
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CHXII03:ELECTROCHEMISTRY

330420 Calculate standard free energy change (in kilojoules) for the reaction,\({\mathrm{\dfrac{1}{2} \mathrm{Cu}_{(s)}+\dfrac{1}{2} \mathrm{Cl}_{2(g)} \rightleftharpoons \dfrac{1}{2} \mathrm{Cu}^{2+}+\mathrm{Cl}^{-}}}\) taking place at \({\mathrm{25{ }^{\circ} \mathrm{C}}}\) in a cell whose standard e.m.f. is 1.02 volts. \({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

1 \( - 98.43\)
2 98.43
3 \( - 965\)
4 965
CHXII03:ELECTROCHEMISTRY

330421 For a relation \({{\rm{\Delta }}_{\rm{r}}}{\rm{G = - nF}}{{\rm{E}}_{{\rm{cell}}}}{\rm{;}}{{\rm{E}}_{{\rm{cell}}}}{\rm{ = E}}_{{\rm{cell}}}^{\rm{o}}\) in which of the following condition?

1 Concentration of any one of the reacting species should be unity
2 Concentration of all the product species should be unity
3 Concentration of all the reacting species should be unity
4 Concentration of all reacting and product species should be unity.
CHXII03:ELECTROCHEMISTRY

330422 \(\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\) for the cell with cell reaction:
\({\text{Zn(s) + A}}{{\text{g}}_{\text{2}}}{\text{O(s) + }}{{\text{H}}_{\text{2}}}{\text{O (l) }} \to \)
\(\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}_{(\mathrm{s})}+2 \mathrm{OH}^{-}(\mathrm{aq})\), is
\(\left[\mathrm{E}_{\mathrm{Ag}_{2} \mathrm{O} \mid \mathrm{Ag}}^{\circ}=+0.344 \mathrm{~V}, \mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{\circ}=-0.76 \mathrm{~V}\right]\)

1 \(2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
2 \(-2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
3 \(1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
4 \(-1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
CHXII03:ELECTROCHEMISTRY

330423 For the electrochemical cell : \({\mathrm{M\left \vert M^{2+} \vert X\right \vert X^{2-}}}\) If, \({\mathrm{\mathrm{E}_{\left(\mathrm{M}^{2+} / \mathrm{M}\right)}^{\circ}=0.46 \mathrm{~V}}}\) and \({\mathrm{\mathrm{E}_{\left(\mathrm{x} / \mathrm{x}^{2-}\right)}^{\circ}=0.34 \mathrm{~V}}}\).
Which of the following is correct?

1 \({\mathrm{M^{2+}+X^{2-} \rightarrow M+X}}\) is a spontaneous reaction.
2 \({\mathrm{\mathrm{M}+\mathrm{X} \rightarrow \mathrm{M}^{2+}+\mathrm{X}^{2-}}}\) is a spontaneous reaction.
3 \({\mathrm{\mathrm{E}_{\text {cell }}=0.80 \mathrm{~V}}}\)
4 \({\mathrm{\mathrm{E}_{\text {cell }}=-0.80 \mathrm{~V}}}\)
JEE Main - 2024
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330420 Calculate standard free energy change (in kilojoules) for the reaction,\({\mathrm{\dfrac{1}{2} \mathrm{Cu}_{(s)}+\dfrac{1}{2} \mathrm{Cl}_{2(g)} \rightleftharpoons \dfrac{1}{2} \mathrm{Cu}^{2+}+\mathrm{Cl}^{-}}}\) taking place at \({\mathrm{25{ }^{\circ} \mathrm{C}}}\) in a cell whose standard e.m.f. is 1.02 volts. \({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

1 \( - 98.43\)
2 98.43
3 \( - 965\)
4 965
CHXII03:ELECTROCHEMISTRY

330421 For a relation \({{\rm{\Delta }}_{\rm{r}}}{\rm{G = - nF}}{{\rm{E}}_{{\rm{cell}}}}{\rm{;}}{{\rm{E}}_{{\rm{cell}}}}{\rm{ = E}}_{{\rm{cell}}}^{\rm{o}}\) in which of the following condition?

1 Concentration of any one of the reacting species should be unity
2 Concentration of all the product species should be unity
3 Concentration of all the reacting species should be unity
4 Concentration of all reacting and product species should be unity.
CHXII03:ELECTROCHEMISTRY

330422 \(\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\) for the cell with cell reaction:
\({\text{Zn(s) + A}}{{\text{g}}_{\text{2}}}{\text{O(s) + }}{{\text{H}}_{\text{2}}}{\text{O (l) }} \to \)
\(\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}_{(\mathrm{s})}+2 \mathrm{OH}^{-}(\mathrm{aq})\), is
\(\left[\mathrm{E}_{\mathrm{Ag}_{2} \mathrm{O} \mid \mathrm{Ag}}^{\circ}=+0.344 \mathrm{~V}, \mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{\circ}=-0.76 \mathrm{~V}\right]\)

1 \(2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
2 \(-2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
3 \(1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
4 \(-1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
CHXII03:ELECTROCHEMISTRY

330423 For the electrochemical cell : \({\mathrm{M\left \vert M^{2+} \vert X\right \vert X^{2-}}}\) If, \({\mathrm{\mathrm{E}_{\left(\mathrm{M}^{2+} / \mathrm{M}\right)}^{\circ}=0.46 \mathrm{~V}}}\) and \({\mathrm{\mathrm{E}_{\left(\mathrm{x} / \mathrm{x}^{2-}\right)}^{\circ}=0.34 \mathrm{~V}}}\).
Which of the following is correct?

1 \({\mathrm{M^{2+}+X^{2-} \rightarrow M+X}}\) is a spontaneous reaction.
2 \({\mathrm{\mathrm{M}+\mathrm{X} \rightarrow \mathrm{M}^{2+}+\mathrm{X}^{2-}}}\) is a spontaneous reaction.
3 \({\mathrm{\mathrm{E}_{\text {cell }}=0.80 \mathrm{~V}}}\)
4 \({\mathrm{\mathrm{E}_{\text {cell }}=-0.80 \mathrm{~V}}}\)
JEE Main - 2024
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CHXII03:ELECTROCHEMISTRY

330420 Calculate standard free energy change (in kilojoules) for the reaction,\({\mathrm{\dfrac{1}{2} \mathrm{Cu}_{(s)}+\dfrac{1}{2} \mathrm{Cl}_{2(g)} \rightleftharpoons \dfrac{1}{2} \mathrm{Cu}^{2+}+\mathrm{Cl}^{-}}}\) taking place at \({\mathrm{25{ }^{\circ} \mathrm{C}}}\) in a cell whose standard e.m.f. is 1.02 volts. \({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

1 \( - 98.43\)
2 98.43
3 \( - 965\)
4 965
CHXII03:ELECTROCHEMISTRY

330421 For a relation \({{\rm{\Delta }}_{\rm{r}}}{\rm{G = - nF}}{{\rm{E}}_{{\rm{cell}}}}{\rm{;}}{{\rm{E}}_{{\rm{cell}}}}{\rm{ = E}}_{{\rm{cell}}}^{\rm{o}}\) in which of the following condition?

1 Concentration of any one of the reacting species should be unity
2 Concentration of all the product species should be unity
3 Concentration of all the reacting species should be unity
4 Concentration of all reacting and product species should be unity.
CHXII03:ELECTROCHEMISTRY

330422 \(\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\) for the cell with cell reaction:
\({\text{Zn(s) + A}}{{\text{g}}_{\text{2}}}{\text{O(s) + }}{{\text{H}}_{\text{2}}}{\text{O (l) }} \to \)
\(\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}_{(\mathrm{s})}+2 \mathrm{OH}^{-}(\mathrm{aq})\), is
\(\left[\mathrm{E}_{\mathrm{Ag}_{2} \mathrm{O} \mid \mathrm{Ag}}^{\circ}=+0.344 \mathrm{~V}, \mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{\circ}=-0.76 \mathrm{~V}\right]\)

1 \(2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
2 \(-2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
3 \(1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
4 \(-1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
CHXII03:ELECTROCHEMISTRY

330423 For the electrochemical cell : \({\mathrm{M\left \vert M^{2+} \vert X\right \vert X^{2-}}}\) If, \({\mathrm{\mathrm{E}_{\left(\mathrm{M}^{2+} / \mathrm{M}\right)}^{\circ}=0.46 \mathrm{~V}}}\) and \({\mathrm{\mathrm{E}_{\left(\mathrm{x} / \mathrm{x}^{2-}\right)}^{\circ}=0.34 \mathrm{~V}}}\).
Which of the following is correct?

1 \({\mathrm{M^{2+}+X^{2-} \rightarrow M+X}}\) is a spontaneous reaction.
2 \({\mathrm{\mathrm{M}+\mathrm{X} \rightarrow \mathrm{M}^{2+}+\mathrm{X}^{2-}}}\) is a spontaneous reaction.
3 \({\mathrm{\mathrm{E}_{\text {cell }}=0.80 \mathrm{~V}}}\)
4 \({\mathrm{\mathrm{E}_{\text {cell }}=-0.80 \mathrm{~V}}}\)
JEE Main - 2024
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CHXII03:ELECTROCHEMISTRY

330420 Calculate standard free energy change (in kilojoules) for the reaction,\({\mathrm{\dfrac{1}{2} \mathrm{Cu}_{(s)}+\dfrac{1}{2} \mathrm{Cl}_{2(g)} \rightleftharpoons \dfrac{1}{2} \mathrm{Cu}^{2+}+\mathrm{Cl}^{-}}}\) taking place at \({\mathrm{25{ }^{\circ} \mathrm{C}}}\) in a cell whose standard e.m.f. is 1.02 volts. \({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

1 \( - 98.43\)
2 98.43
3 \( - 965\)
4 965
CHXII03:ELECTROCHEMISTRY

330421 For a relation \({{\rm{\Delta }}_{\rm{r}}}{\rm{G = - nF}}{{\rm{E}}_{{\rm{cell}}}}{\rm{;}}{{\rm{E}}_{{\rm{cell}}}}{\rm{ = E}}_{{\rm{cell}}}^{\rm{o}}\) in which of the following condition?

1 Concentration of any one of the reacting species should be unity
2 Concentration of all the product species should be unity
3 Concentration of all the reacting species should be unity
4 Concentration of all reacting and product species should be unity.
CHXII03:ELECTROCHEMISTRY

330422 \(\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\) for the cell with cell reaction:
\({\text{Zn(s) + A}}{{\text{g}}_{\text{2}}}{\text{O(s) + }}{{\text{H}}_{\text{2}}}{\text{O (l) }} \to \)
\(\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}_{(\mathrm{s})}+2 \mathrm{OH}^{-}(\mathrm{aq})\), is
\(\left[\mathrm{E}_{\mathrm{Ag}_{2} \mathrm{O} \mid \mathrm{Ag}}^{\circ}=+0.344 \mathrm{~V}, \mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{\circ}=-0.76 \mathrm{~V}\right]\)

1 \(2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
2 \(-2.13 \times 10^{5} \mathrm{Jmol}^{-1}\)
3 \(1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
4 \(-1.06 \times 10^{5} \mathrm{Jmol}^{-1}\)
CHXII03:ELECTROCHEMISTRY

330423 For the electrochemical cell : \({\mathrm{M\left \vert M^{2+} \vert X\right \vert X^{2-}}}\) If, \({\mathrm{\mathrm{E}_{\left(\mathrm{M}^{2+} / \mathrm{M}\right)}^{\circ}=0.46 \mathrm{~V}}}\) and \({\mathrm{\mathrm{E}_{\left(\mathrm{x} / \mathrm{x}^{2-}\right)}^{\circ}=0.34 \mathrm{~V}}}\).
Which of the following is correct?

1 \({\mathrm{M^{2+}+X^{2-} \rightarrow M+X}}\) is a spontaneous reaction.
2 \({\mathrm{\mathrm{M}+\mathrm{X} \rightarrow \mathrm{M}^{2+}+\mathrm{X}^{2-}}}\) is a spontaneous reaction.
3 \({\mathrm{\mathrm{E}_{\text {cell }}=0.80 \mathrm{~V}}}\)
4 \({\mathrm{\mathrm{E}_{\text {cell }}=-0.80 \mathrm{~V}}}\)
JEE Main - 2024
NEET DIGITAL LIBRARY