MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Secondary Cells

During the di...

Question

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 g $m l^{- 1}$ and sulphuric acid of the density of 1.294 g $m l^{- 1}$ is 39% by mass and that of the density of 1.139 g $m l^{- 1}$ is 20% by mass. The battery holds 3.5 litre of acid and the volume practically remained constant during the discharge. Calculate the no. of ampere hour 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

A

2.5 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!

B

1.7 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

3.2 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

None of these

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D None of these
Initial mass of $H_{2} S O_{4} = 1.294 \times \frac{39}{100} \times 3.5 = 1766 g m$

Final mass of $H_{2} S O_{4} = 1.139 \times \frac{20}{100} \times 3.5 = 797 g m$

Mass of $H_{2} S O_{4}$ electrolyzed= $(1766 - 797) \approx 980 g m$

$96500 C$ charge electrolyzes 49 gm of $H_{2} S O_{4}$

$980 g m H_{2} S O_{4}$ is electrolysed by $\frac{96500 \times 980}{49} C$ charge

Ampere hours required $\frac{96500 \times 980}{49 \times 60 \times 60} = 536 C / h r$

Suggest Corrections

thumbs-up

0

Similar questions

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 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^{-}

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. 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}

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^{-}

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

Q. During the discharge of a lead storage battery, density of

H_{2} S O_{4}

1.294

1.139

. S u l p h u r i c a c i d o f d e n s i t y

i s

b y w e i g h t a n d t h a t o f d e n s i t y

i s

b y w e i g h t . T h e b a t t e r y h o l d

o f t h e a c i d a n d v o l u m e r e m a i n s p r a c t i c a l l y c o n s t a n t d u r i n g d i s c h a r g e . C a l c u l a t e a m p e r e - h o u r o f w h i c h t h e b a t t e r y m u s t h a v e b e e n u s e d . T h e c h a r g i n g a n d d i s c h a r g i n g r e a c t i o n s a r e :

Pb + SO_{4}^{2-} \rightarrow PbSO_{4} + 2e^{-}

(c h a r g i n g)

PbO_{2} + 4H^{+} + SO_{4}^{2-} + 2e^{-}\rightarrow PbSO_{4} + 2H_{2}O$ (discharging).

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)

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Secondary Cells

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Secondary Cells

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon