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Standard XII

Chemistry

Faraday's Second Law

In a fuel cel...

Question

In a fuel cell $H_{2}$ and $O_{2}$ react to product electricity. In the process, hydrogen is oxidized at anode and oxygen at cathode. If 67.2 l of $H_{2}$ at STP reacts in 15 min, the average current produced ( $i n A$ ) is_______. (nearest value)

Anode : $H_{2} + 2 ⊖ O H \to 2 H_{2} O + 2 e^{-}$
Cathode : $O_{2} + 2 H_{2}) + 2 e^{-} \to 4 ⊖ O H$

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Solution

Anode : $H_{2} + 2 ⊖ O H \to 2 H_{2} O + 2 e^{-}$

Volume of $H_{2}$ reacts in 15 min = 67.2 L

Moles of $H_{2} = \frac{67.2}{22.4} = 3 m o l$

2 F $= 1 m o l H_{2}$

$\Rightarrow$ 3 mol $H_{2} = 6 F$

$\Rightarrow \frac{I \times 15 \times 60}{96500} = 6$

$\Rightarrow I = 643.33 A \approx 643 A$

$C u^{2 +} + 2 e^{-} \to C u$

2 F = 1 mol Cu
6 F = 3 mol Cu

$\Rightarrow$ Grams of Cu deposite $= 3 \times 63.5 = 190.5 g$

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Similar questions

In a fuel cell, hydrogen and oxygen react to produce electricity. In the process, hydrogen gas is oxidized at anode and oxygen at cathode. If 67.2 L of $H_{2}$ at STP reacts in 15 min, the average current (in A) produced is :

Anode reaction : $H_{2} + 2 ⊖ O H \to 2 H_{2} O + 2 e^{-}$

Cathode reaction :

O_{2} + 2 H_{2} O + 2 e^{-} \to 4 ⊖ O H

(write your answer to nearest integer)

Q. In a fuel cell

H_{2}

and

O_{2}

react to produce electricity. In the process

H_{2}

gas is oxidized at anode and

O_{2}

at cathode. If 67.2 litre of

H_{2}

at STP reacts in 15 minutes. The average current produced is:

Q. In a fuel cell,

H_{2}

and

O_{2}

react to produce electricity. In the process,

H_{2}

gas is oxidized at the anode and

O_{2}

gas is reduced at the cathode. If

67.2 litres

H_{2}

S T P

react in 15 minutes and the entire current is used for electrode deposition of

C u

from

C u (I I)

solution, how many grams of

C u

will be deposited and what is the average current produced?
Anode :

H_{2} + 2 O H^{-} \to 2 H_{2} O + 2 e^{-}

Cathode :

O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}

Q. In a fuel cell,

H_{2}

and

O_{2}

react to produce electricity. In the process,

H_{2}

gas is oxidized at the anode and

O_{2}

gas is reduced at the cathode. If

67.2 litres

H_{2}

S T P

react in 15 minutes and the entire current is used for electrode deposition of

C u

from

C u (I I)

solution, how many grams of

C u

will be deposited and what is the average current produced?
Anode :

H_{2} + 2 O H^{-} \to 2 H_{2} O + 2 e^{-}

Cathode :

O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}

Q. In a fuel cell,

H_{2}

and

O_{2}

react to produce electricity. In the process

H_{2}

gas is oxidised at the anode and

O_{2}

is reduced at the cathode. If

67.2 L

H_{2}

S T P

reacts in

15 m i n

, what is the average currecnt produced? If the entire current is used for electro deposition of

C u

from

C u^{2 +}

, how many grams of

C u

are deposited?

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In a fuel cell H2 and O2 react to product electricity. In the process, hydrogen is oxidized at anode and oxygen at cathode. If 67.2 l of H2 at STP reacts in 15 min, the average current produced (inA) is_______. (nearest value)Anode : H2+2⊖OH→2H2O+2e−Cathode : O2+2H2)+2e−→4⊖OH

Anode : H2+2⊖OH→2H2O+2e−Volume of H2 reacts in 15 min = 67.2 LMoles of H2=67.222.4=3mol2 F =1molH2⇒ 3 mol H2=6F⇒I×15×6096500=6⇒I=643.33A≈643 ACu2++2e−→Cu2 F = 1 mol Cu6 F = 3 mol Cu⇒ Grams of Cu deposite =3×63.5=190.5g