In which cell,construction like a galvanic cell can be observed? Explain.
(N/A) fuel cell is a device that converts chemical energy directly into electrical energy and possesses a construction similar to a galvanic cell.
Construction: In fuel cells,reactants are fed continuously to the electrodes,and products are removed continuously from the electrolyte compartment. These cells are designed to convert the energy of combustion of fuels like $H_2$,$CH_4$,or $CH_3OH$ directly into electrical energy.
Advantages of fuel cells:
$(i)$ There is no air or noise pollution.
$(ii)$ Fuel cells have high efficiency of $70 \%$ or more,whereas thermal power stations have low efficiency of $40 \%$ or less.
$(iii)$ Various types of fuels can be used in fuel cells.
Construction: In fuel cells,reactants are fed continuously to the electrodes,and products are removed continuously from the electrolyte compartment. These cells are designed to convert the energy of combustion of fuels like $H_2$,$CH_4$,or $CH_3OH$ directly into electrical energy.
Advantages of fuel cells:
$(i)$ There is no air or noise pollution.
$(ii)$ Fuel cells have high efficiency of $70 \%$ or more,whereas thermal power stations have low efficiency of $40 \%$ or less.
$(iii)$ Various types of fuels can be used in fuel cells.
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Similar Questions
In the cell represented as $Ni_{(s)}|Ni_{(1M)}^{2+}||Ag_{(1M)}^{+}|Ag_{(s)}$,the reducing agent is
The standard reduction potential data at $25^{\circ} C$ is given below.
$E^{\circ}(Fe^{3+}, Fe^{2+}) = +0.77 \ V$
$E^{\circ}(Fe^{2+}, Fe) = -0.44 \ V$
$E^{\circ}(Cu^{2+}, Cu) = +0.34 \ V$
$E^{\circ}(Cu^{+}, Cu) = +0.52 \ V$
$E^{\circ}(O_{2(g)} + 4H^{+} + 4e^{-} \rightarrow 2H_{2}O) = +1.23 \ V$
$E^{\circ}(O_{2(g)} + 2H_{2}O + 4e^{-} \rightarrow 4OH^{-}) = +0.40 \ V$
$E^{\circ}(Cr^{3+}, Cr) = -0.74 \ V$
$E^{\circ}(Cr^{2+}, Cr) = -0.91 \ V$
Match $E^{\circ}$ of the redox pair in List-$I$ with the values given in List-$II$ and select the correct answer using the code given below the lists:
List-$I$ List-$II$ $P. \ E^{\circ}(Fe^{3+}, Fe)$ $1. \ -0.18 \ V$ $Q. \ E^{\circ}(4H_{2}O \rightleftharpoons 4H^{+} + 4OH^{-})$ $2. \ -0.4 \ V$ $R. \ E^{\circ}(Cu^{2+} + Cu \rightarrow 2Cu^{+})$ $3. \ -0.04 \ V$ $S. \ E^{\circ}(Cr^{3+}, Cr^{2+})$ $4. \ -0.83 \ V$
Codes: $P \quad Q \quad R \quad S$
$E^{\circ}(Fe^{3+}, Fe^{2+}) = +0.77 \ V$
$E^{\circ}(Fe^{2+}, Fe) = -0.44 \ V$
$E^{\circ}(Cu^{2+}, Cu) = +0.34 \ V$
$E^{\circ}(Cu^{+}, Cu) = +0.52 \ V$
$E^{\circ}(O_{2(g)} + 4H^{+} + 4e^{-} \rightarrow 2H_{2}O) = +1.23 \ V$
$E^{\circ}(O_{2(g)} + 2H_{2}O + 4e^{-} \rightarrow 4OH^{-}) = +0.40 \ V$
$E^{\circ}(Cr^{3+}, Cr) = -0.74 \ V$
$E^{\circ}(Cr^{2+}, Cr) = -0.91 \ V$
Match $E^{\circ}$ of the redox pair in List-$I$ with the values given in List-$II$ and select the correct answer using the code given below the lists:
| List-$I$ | List-$II$ |
| $P. \ E^{\circ}(Fe^{3+}, Fe)$ | $1. \ -0.18 \ V$ |
| $Q. \ E^{\circ}(4H_{2}O \rightleftharpoons 4H^{+} + 4OH^{-})$ | $2. \ -0.4 \ V$ |
| $R. \ E^{\circ}(Cu^{2+} + Cu \rightarrow 2Cu^{+})$ | $3. \ -0.04 \ V$ |
| $S. \ E^{\circ}(Cr^{3+}, Cr^{2+})$ | $4. \ -0.83 \ V$ |
Codes: $P \quad Q \quad R \quad S$
The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:
MediumIIT 1985
View SolutionCan you store copper sulphate solutions in a zinc pot?
Medium
View SolutionStandard electrode potentials for a few half cells are mentioned below:
$E^0_{Cu^{2+}/Cu} = 0.34 \ V, E^0_{Zn^{2+}/Zn} = -0.76 \ V$
$E^0_{Ag^{+}/Ag} = 0.80 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$
Which one of the following cells gives the most negative value of $\Delta G^0$?
$E^0_{Cu^{2+}/Cu} = 0.34 \ V, E^0_{Zn^{2+}/Zn} = -0.76 \ V$
$E^0_{Ag^{+}/Ag} = 0.80 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$
Which one of the following cells gives the most negative value of $\Delta G^0$?
DifficultJEE MAIN 2025
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