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Standard X

Chemistry

Electrolytic Cell

The anodic ha...

Question

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of $P b S O_{4}$ electrolysed in g during the process is:(molar mass of $P b S O_{4}$ =303 g ${mol}^{- 1}$ )

22.8

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15.2

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7.6

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11.4

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Solution

The correct option is B 15.2
$(Anode) {PbSO}_{4} (s) + 2 {OH}^{-} \to {PbO}_{2} + H_{2} {SO}_{4} + 2 e^{-} 0.05 / 2 mole 0.05 F (Cathode) {PbSO}_{4} + 2 e^{-} + 2 H^{+} \to Pb (s) + H_{2} {SO}_{4} 0.05 / 2 mole 0.05 F n_{T} ({PbSO}_{4}) = 0.05 \times 303 = 15.2 g$

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Similar questions

Q. The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of

P b S O_{4}

electrolysed in g during the process is:(molar mass of

P b S O_{4}

=303 g

{mol}^{- 1}

)

Q. During the discharge of a lead storage battery the density of sulphuric acid fell from

1.294

1.139 {g mL}^{- 1}

H_{2} S O_{4}

of density

1.294 {g mL}^{- 1}

is 39% and that of density

1.139 {g mL}^{- 1}

is 20% by weight. The battery holds

3.5 L

of acid and the volume practically remains constant during the discharge. Calculate the number of Ampere hours for which the battery must have been used. The discharging reactions are:

P b + S O_{4}^{2 -} \to P b S O_{4} + 2 e^{-} (anode)

P b O_{2} + 4 H^{+} + S O_{4}^{2 -} + 2 e^{-} \to P b S O_{4} + 2 H_{2} O (cathode)

Q. During the discharge of a lead storage battery, the density of sulphuric acid fell from

1.294

1.139 {g mL}^{- 1}

. Sulphuric acid of density

1.294 {g mL}^{- 1}

39 % H_{2} S O_{4}

by mass and that of density

1.139 {g mL}^{- 1}

20 % H_{2} S O_{4}

by mass. The battery holds

3.5 L

of the acid and the volume remained practically constant during the discharge. The charging and discharging reactions are

P b + S O_{4}^{2 -} \to P b S O_{4} + 2 e^{-}

(charging)

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

(discharging)
The number of ampere-hour for which the battery must have been used is

Q. In a lead storage battery, the anode reaction is,

P b + H_{2} S O_{4} \to P b S O_{4} + 2 H^{+} + 2 e^{-}

Weight in g of Pb would be used up for battery to use for 1 ampere hour is___________. (write the nearest integer value)

Q. During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139

g m L^{- 1}

H_{2} S O_{4}

of density

1.294 g m L^{- 1}

is 39% and that of density

1.139 g m L^{- 1}

is 20% by weight.The battery holds 3.5 L of acid and the volume practically remains constant during discharge. The number of ampere hours for which the battery must have been used are........................
The discharging and charging reactions are:

P b + S O_{4}^{2 -} \to P b S O_{4} + 2 e^{-}

(charging)

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

(discharging)

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The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolysed in g during the process is:(molar mass of PbSO4=303 g mol−1)

The correct option is B 15.2(Anode) PbSO4(s) +2OH−→PbO2 +H2SO4+2e− 0.05/2 mole 0.05F(Cathode) PbSO4+2e− +2H+ →Pb(s)+H2SO4 0.05/2 mole 0.05 F nT(PbSO4) =0.05 ×303 =15.2 g

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of $P b S O_{4}$ electrolysed in g during the process is:(molar mass of $P b S O_{4}$ =303 g ${mol}^{- 1}$ )

The correct option is B 15.2
$(Anode) {PbSO}_{4} (s) + 2 {OH}^{-} \to {PbO}_{2} + H_{2} {SO}_{4} + 2 e^{-} 0.05 / 2 mole 0.05 F (Cathode) {PbSO}_{4} + 2 e^{-} + 2 H^{+} \to Pb (s) + H_{2} {SO}_{4} 0.05 / 2 mole 0.05 F n_{T} ({PbSO}_{4}) = 0.05 \times 303 = 15.2 g$