Consider the following statements pertaining to fuel cells :-
$(a)$ Hydrogen-oxygen fuel cells make use of concentrated $KOH$ solution as an electrolyte and porous graphite impregnated with platinum as electrodes.
$(b)$ The efficiency of a fuel cell is less than unity due to polarization at electrodes and the resistance offered by the electrode and the electrolyte.
$(c)$ The electrical work,assuming the cell to be working reversibly,may be represented as $-\Delta G = W_{\text{electrical}} = -\Delta H + T\Delta S$.
Which of the above statements are correct?
$(a)$ Hydrogen-oxygen fuel cells make use of concentrated $KOH$ solution as an electrolyte and porous graphite impregnated with platinum as electrodes.
$(b)$ The efficiency of a fuel cell is less than unity due to polarization at electrodes and the resistance offered by the electrode and the electrolyte.
$(c)$ The electrical work,assuming the cell to be working reversibly,may be represented as $-\Delta G = W_{\text{electrical}} = -\Delta H + T\Delta S$.
Which of the above statements are correct?
- A$(a)$ and $(b)$
- B$(a)$ and $(c)$
- C$(b)$ and $(c)$
- D$(a), (b)$ and $(c)$
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The molar conductivity of a solution of a weak acid $HX$ $(0.01 \ M)$ is $10$ times smaller than the molar conductivity of a solution of a weak acid $HY$ $(0.10 \ M)$. If $\lambda_{X^{-}}^0 \approx \lambda_{Y^{-}}^0$,the difference in their $pK_a$ values,$pK_a(HX) - pK_a(HY)$,is (consider degree of ionization of both acids to be $\ll 1$)
Consider the following cell reaction:
$Cd_{(s)} + Hg_{2}SO_{4(s)} + \frac{9}{5}H_{2}O_{(l)} \rightleftharpoons CdSO_{4} \cdot \frac{9}{5}H_{2}O_{(s)} + 2Hg_{(l)}$
The value of $E_{\text{cell}}^{0}$ is $4.315 \ V$ at $25^{\circ}C$. If $\Delta H^{\circ} = -825.2 \ kJ \ mol^{-1}$,the standard entropy change $\Delta S^{\circ}$ in $J \ K^{-1} \ mol^{-1}$ is ........ . (Nearest integer) [Given: Faraday constant $= 96487 \ C \ mol^{-1}$]
$Cd_{(s)} + Hg_{2}SO_{4(s)} + \frac{9}{5}H_{2}O_{(l)} \rightleftharpoons CdSO_{4} \cdot \frac{9}{5}H_{2}O_{(s)} + 2Hg_{(l)}$
The value of $E_{\text{cell}}^{0}$ is $4.315 \ V$ at $25^{\circ}C$. If $\Delta H^{\circ} = -825.2 \ kJ \ mol^{-1}$,the standard entropy change $\Delta S^{\circ}$ in $J \ K^{-1} \ mol^{-1}$ is ........ . (Nearest integer) [Given: Faraday constant $= 96487 \ C \ mol^{-1}$]
Which of the following is not correct?
Consider the following data.
Electrolyte $\Lambda_m^\circ$ $(S\text{ cm}^2\text{ mol}^{-1})$ $BaCl_2$ $x_1$ $H_2SO_4$ $x_2$ $HCl$ $x_3$
$BaSO_4$ is sparingly soluble in water. If the conductivity of the saturated $BaSO_4$ solution is $x\text{ S cm}^{-1}$, then the solubility product of $BaSO_4$ can be given as (Here $\Lambda_m = \Lambda_m^\circ$)
| Electrolyte | $\Lambda_m^\circ$ $(S\text{ cm}^2\text{ mol}^{-1})$ |
|---|---|
| $BaCl_2$ | $x_1$ |
| $H_2SO_4$ | $x_2$ |
| $HCl$ | $x_3$ |
$BaSO_4$ is sparingly soluble in water. If the conductivity of the saturated $BaSO_4$ solution is $x\text{ S cm}^{-1}$, then the solubility product of $BaSO_4$ can be given as (Here $\Lambda_m = \Lambda_m^\circ$)
DifficultJEE MAIN 2026
View SolutionMatch List-$I$ with List-$II$.
List-$I$ (Conversion) List-$II$ (Number of Faraday required) $A$. $1 \ mol$ of $H_2O$ to $O_2$ $I$. $3 \ F$ $B$. $1 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$ $II$. $2 \ F$ $C$. $1.5 \ mol$ of $Ca$ from molten $CaCl_2$ $III$. $1 \ F$ $D$. $1 \ mol$ of $FeO$ to $Fe_2O_3$ $IV$. $5 \ F$
Choose the correct answer from the options given below:
| List-$I$ (Conversion) | List-$II$ (Number of Faraday required) |
| $A$. $1 \ mol$ of $H_2O$ to $O_2$ | $I$. $3 \ F$ |
| $B$. $1 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$ | $II$. $2 \ F$ |
| $C$. $1.5 \ mol$ of $Ca$ from molten $CaCl_2$ | $III$. $1 \ F$ |
| $D$. $1 \ mol$ of $FeO$ to $Fe_2O_3$ | $IV$. $5 \ F$ |
Choose the correct answer from the options given below:
MediumNEET 2024
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