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Standard XII

Biology

Pyranose and Furanose

Does the stre...

Question

Does the strength of the sulphuric acid ________ during the discharge of a car battery? Fill in the blank.

Decrease

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Increase

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Remain same

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None of the above

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Solution

The correct option is A Decrease
Discharging reaction : $P b$ $+$ $P b O_{2}$ $+$ $2 H_{2} S O_{4}$ $\to$ $2 P b S O_{4}$ $+$ $2 H_{2} O$
$⟹$ $H_{2} S O_{4}$ gets consumed during discharging of the car battery, hence strength of the sulphuric acid decreases during the discharge of a car battery.

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Similar questions

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

1.294

1.139 g m l^{- 1}

. Sulphuric acid of density

1.294 g m l^{- 1}

is 39% by weight and that of density

1.139 g m l^{- 1}

is 20% by weight. The battery holds 3.5 L of the acid and the volume remained practically constant during the discharge. Find the number of ampere-hours for which the battery must has been used.

The charging and discharging reactions are as follows:

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

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

During the discharge of a lead storage battery, the density of sulphuric acid fell from $1.294$ to $1.139$ gm $L^{- 1}$ . Sulphuric acid of density $1.294$ gm $L^{- 1}$ is $39$ % by weight and that of density 1.139 gm $L^{- 1}$ is $20$ % by weight. The battery holds $3.5$ litres of acid and the column practically remained constant during the discharge.

Calculate the number of ampere-hours for which the battery must have been used. 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)

Q. During discharge of a lead storage cell the density of sulphuric acid in the cell :

Q. During discharge of a lead storage cell, the density of sulphuric acid in the cell:

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

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Does the strength of the sulphuric acid ________ during the discharge of a car battery? Fill in the blank.

The correct option is A DecreaseDischarging reaction : Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O⟹ H2SO4 gets consumed during discharging of the car battery, hence strength of the sulphuric acid decreases during the discharge of a car battery.

The correct option is A Decrease
Discharging reaction : $P b$ $+$ $P b O_{2}$ $+$ $2 H_{2} S O_{4}$ $\to$ $2 P b S O_{4}$ $+$ $2 H_{2} O$
$⟹$ $H_{2} S O_{4}$ gets consumed during discharging of the car battery, hence strength of the sulphuric acid decreases during the discharge of a car battery.