330081
Two half-cells have reduction potentials \({\rm{ - 0}}{\rm{.76 V and - 0}}{\rm{.13 V}}\) respectively. A galvanic cell is made from these two half-cell. Which of the following statements is correct?
1 Electrode half-cell potential –0.13 V serve as anode.
2 Electrode half-cell potential –0.76 V serve as positive electrode and –0.13 V as negative electrode.
3 Electrode half-cell potential –0.76 V serve as cathode.
4 Electrode half-cell potential –0.76 V serve as anode.
Explanation:
The electrode with more negative reduction potential constitutes the anode.
CHXII03:ELECTROCHEMISTRY
330052
The chemical reaction, \(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) taking place in a galvanic cell is represented by the notation.
\(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g})(1 \mathrm{bar}) \rightarrow\) \(2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) The cell with this cell reaction can be represented by \(\mathop {\operatorname{Pt} ({\text{s}})}\limits_{{\text{ (anode) }}} \left \vert {{{\text{H}}_2}(\;{\text{g}})(1\,{\text{bar}})} \right \vert 1{\text{M HCl}}({\text{aq}}),\) \(\left \vert {\left \vert {\mathop {{{\operatorname{Ag} }^ + }({\text{aq}})}\limits_{{\text{ (cathode) }}} } \right \vert } \right \vert \operatorname{Ag} ({\text{s}})\) Silver is undergoing reduction \(\left(\mathrm{Ag}^{+} \rightarrow \mathrm{Ag}\right)\) in this reaction, hence, it will act as cathode in the cell. Option (1) has \(\mathrm{KCl}\) which is not present in the cell, so it is incorrect. Option (3) has \(\mathrm{AgCl}(\mathrm{s})\) and \(\mathrm{AgCl}\) do not ionise, it is also incorrect. Option (4) at cathode Ag is being oxidised to \(\mathrm{Ag}^{+}\)but at cathode, oxidation does not take place hence, it is also incorrect. Hence, option (2) is correct.
330081
Two half-cells have reduction potentials \({\rm{ - 0}}{\rm{.76 V and - 0}}{\rm{.13 V}}\) respectively. A galvanic cell is made from these two half-cell. Which of the following statements is correct?
1 Electrode half-cell potential –0.13 V serve as anode.
2 Electrode half-cell potential –0.76 V serve as positive electrode and –0.13 V as negative electrode.
3 Electrode half-cell potential –0.76 V serve as cathode.
4 Electrode half-cell potential –0.76 V serve as anode.
Explanation:
The electrode with more negative reduction potential constitutes the anode.
CHXII03:ELECTROCHEMISTRY
330052
The chemical reaction, \(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) taking place in a galvanic cell is represented by the notation.
\(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g})(1 \mathrm{bar}) \rightarrow\) \(2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) The cell with this cell reaction can be represented by \(\mathop {\operatorname{Pt} ({\text{s}})}\limits_{{\text{ (anode) }}} \left \vert {{{\text{H}}_2}(\;{\text{g}})(1\,{\text{bar}})} \right \vert 1{\text{M HCl}}({\text{aq}}),\) \(\left \vert {\left \vert {\mathop {{{\operatorname{Ag} }^ + }({\text{aq}})}\limits_{{\text{ (cathode) }}} } \right \vert } \right \vert \operatorname{Ag} ({\text{s}})\) Silver is undergoing reduction \(\left(\mathrm{Ag}^{+} \rightarrow \mathrm{Ag}\right)\) in this reaction, hence, it will act as cathode in the cell. Option (1) has \(\mathrm{KCl}\) which is not present in the cell, so it is incorrect. Option (3) has \(\mathrm{AgCl}(\mathrm{s})\) and \(\mathrm{AgCl}\) do not ionise, it is also incorrect. Option (4) at cathode Ag is being oxidised to \(\mathrm{Ag}^{+}\)but at cathode, oxidation does not take place hence, it is also incorrect. Hence, option (2) is correct.
330081
Two half-cells have reduction potentials \({\rm{ - 0}}{\rm{.76 V and - 0}}{\rm{.13 V}}\) respectively. A galvanic cell is made from these two half-cell. Which of the following statements is correct?
1 Electrode half-cell potential –0.13 V serve as anode.
2 Electrode half-cell potential –0.76 V serve as positive electrode and –0.13 V as negative electrode.
3 Electrode half-cell potential –0.76 V serve as cathode.
4 Electrode half-cell potential –0.76 V serve as anode.
Explanation:
The electrode with more negative reduction potential constitutes the anode.
CHXII03:ELECTROCHEMISTRY
330052
The chemical reaction, \(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) taking place in a galvanic cell is represented by the notation.
\(2 \mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g})(1 \mathrm{bar}) \rightarrow\) \(2 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) The cell with this cell reaction can be represented by \(\mathop {\operatorname{Pt} ({\text{s}})}\limits_{{\text{ (anode) }}} \left \vert {{{\text{H}}_2}(\;{\text{g}})(1\,{\text{bar}})} \right \vert 1{\text{M HCl}}({\text{aq}}),\) \(\left \vert {\left \vert {\mathop {{{\operatorname{Ag} }^ + }({\text{aq}})}\limits_{{\text{ (cathode) }}} } \right \vert } \right \vert \operatorname{Ag} ({\text{s}})\) Silver is undergoing reduction \(\left(\mathrm{Ag}^{+} \rightarrow \mathrm{Ag}\right)\) in this reaction, hence, it will act as cathode in the cell. Option (1) has \(\mathrm{KCl}\) which is not present in the cell, so it is incorrect. Option (3) has \(\mathrm{AgCl}(\mathrm{s})\) and \(\mathrm{AgCl}\) do not ionise, it is also incorrect. Option (4) at cathode Ag is being oxidised to \(\mathrm{Ag}^{+}\)but at cathode, oxidation does not take place hence, it is also incorrect. Hence, option (2) is correct.