(C) The oxidation reaction at the anode is: $H_2(g) \rightarrow 2H^+(aq) + 2e^-$. Number of moles of $H_2 = \frac{67.2 \ L}{22.4 \ L/mol} = 3 \ mol$.

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(C) The oxidation reaction at the anode is: $H_2(g) \rightarrow 2H^+(aq) + 2e^-$. Number of moles of $H_2 = \frac{67.2 \ L}{22.4 \ L/mol} = 3 \ mol$. Since $2 \ mol$ of electrons are produced per mole of $H_2$,total moles of electrons $(n)$ = $3 \times 2 = 6 \ mol$. Total charge $(Q)$ = $n \times F = 6 \times 96500 \ C = 579000 \ C$. Time $(t)$ = $15 \ min = 15 \times 60 \ s = 900 \ s$. Current $(I)$ = $\frac{Q}{t} = \frac{579000 \ C}{900 \ s} = 643.33 \ A$.

Class 12 Chemistry Electrochemistry Electrochemical cells

Medium

In a fuel cell,$H_2$ and $O_2$ react to produce electricity. In this process,$H_2$ gas is oxidized at the anode and $O_2$ gas is reduced at the cathode. If $67.2 \ L$ of $H_2$ gas at $\text{STP}$ is consumed in $15 \ min$,what is the current produced (in $A$)?

A
$64.33$
B
$6.433$
C
$643.33$
D
$38.6$

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Class 12

Chemistry Questions

Chapter

Electrochemistry

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Electrochemical cells

Which relation is correct for $\Lambda^0_{m(H_2O)}$?

MediumGUJCET 2025

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Match List-$I$ with List-$II$.

$LIST$-$I$ (Cell) $LIST$-$II$ (Use/Property/Reaction)

$A$. Leclanche cell $I$. Converts energy of combustion into electrical energy

$B$. Ni-Cd cell $II$. Does not involve any ion in solution and is used in hearing aids

$C$. Fuel cell $III$. Rechargeable

$D$. Mercury cell $IV$. Reaction at anode $Zn \rightarrow Zn^{2+} + 2e^-$

Choose the correct answer from the options given below:

MediumJEE MAIN 2024

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The $emf$ of the cell reaction is $1.1 \ V$. Calculate the free energy change for the reaction in $kJ$:
$Zn_{(s)} + Cu^{+2}_{(aq)} \longrightarrow Zn^{+2}_{(aq)} + Cu_{(s)}$

Easy

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Which statement is incorrect for a galvanic cell?

Easy

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Derive the relation between the dissociation constant $K_a$ and the limiting molar conductivity $\Lambda_m^o$ for a solution of a weak electrolyte.

Medium

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$LIST$-$I$ (Cell)	$LIST$-$II$ (Use/Property/Reaction)
$A$. Leclanche cell	$I$. Converts energy of combustion into electrical energy
$B$. Ni-Cd cell	$II$. Does not involve any ion in solution and is used in hearing aids
$C$. Fuel cell	$III$. Rechargeable
$D$. Mercury cell	$IV$. Reaction at anode $Zn \rightarrow Zn^{2+} + 2e^-$

In a fuel cell,$H_2$ and $O_2$ react to produce electricity. In this process,$H_2$ gas is oxidized at the anode and $O_2$ gas is reduced at the cathode. If $67.2 \ L$ of $H_2$ gas at $\text{STP}$ is consumed in $15 \ min$,what is the current produced (in $A$)?

Similar Questions

Which relation is correct for $\Lambda^0_{m(H_2O)}$?

The $emf$ of the cell reaction is $1.1 \ V$. Calculate the free energy change for the reaction in $kJ$: $Zn_{(s)} + Cu^{+2}_{(aq)} \longrightarrow Zn^{+2}_{(aq)} + Cu_{(s)}$

Which statement is incorrect for a galvanic cell?

Derive the relation between the dissociation constant $K_a$ and the limiting molar conductivity $\Lambda_m^o$ for a solution of a weak electrolyte.

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The $emf$ of the cell reaction is $1.1 \ V$. Calculate the free energy change for the reaction in $kJ$:
$Zn_{(s)} + Cu^{+2}_{(aq)} \longrightarrow Zn^{+2}_{(aq)} + Cu_{(s)}$