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Fuel Cells

In a hydrogen...

Question

In a hydrogen oxygen fuel cell, electricity is produced. In this process $H_{2} (g)$ is oxidised at anode and $O_{2} (g)$ reduced at cathode.

Given: Cathode $O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)$

Anode $H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}$

4.48 litre $H_{2}$ at 1 atm and 273K oxidised in 9650 sec.

The mass of water produced is:

A

7.2g

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B

3.6g

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C

1.8g

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D

0.9g

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Solution

The correct option is B 3.6g
Mass of $H_{2} O = \frac{4.48}{22.4} \times 18 = 3.6 g$

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Similar questions

Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode.

Given: Cathode

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

H_{2}

at 1 atm and 273K oxidised in 9650 sec.

The current produced is (in amp):

Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode. Given : Cathode:

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

273 K

9650 sec

.
The mass of water produced is (in grams):

Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode. Given : Cathode:

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

273 K

9650 sec

.
The mass of water produced is (in grams):

Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode.
Given : Cathode:

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

273 K

9650 sec

.
The current produced is (in amp):

Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode.
Given : Cathode:

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

273 K

9650 sec

.
The current produced is (in amp):

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