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Application of Electrolysis

Which of the ...

Question

Which of the following reactions are TRUE in case of Lead storage battery?

A

At anode:

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

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B

At cathode:

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

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C

Overall:

P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (s)

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D

None of these.

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Solution

The correct options are
A At anode: $P b (s) + S O_{4}^{2 -} (a q) \to P b S O_{4} (s) + 2 e^{-}$
B At cathode: $P b O_{2} (s) + S O_{4}^{2 -} (a q) + 4 H^{+} (a q) + 2 e^{-} \to P b S O_{4} (s) + 2 H_{2} O (s)$
C Overall:
$P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (s)$
Let's look at the reactions happening in the cell.
The electrode reactions that occur during discharge (i.e., when the external circuit is closed) are as follows:
At anode: $P b (s) + S O_{4}^{2 -} (a q) \to P b S O_{4} (s) + 2 e^{-}$
At cathode: $P b O_{2} (s) + S O_{4}^{2 -} + 4 H^{+} (a q) + 2 e^{-} \to P b S O_{4} (s) + 2 H_{2} O$
Overall reaction
$P b (s) + P b O_{2} (s) + 4 H^{+} (a q) + 2 S O_{4}^{2 -} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O$

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Similar questions

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. Match the column I with column II and mark the appropriate choice.

	Column I		Column II
(A)	$P b_{(s)} + S O_{4 (a q)}^{- 2} \to P b S O_{4 (s)} + 2 e^{-}$	(i)	Rusting of iron
(B)	$2 S O_{4 (a q)}^{2 -} \to S_{2} O_{8 (a q)}^{2 -} + 2 e^{-}$	(ii)	Reaction at anode in lead storage battery
(C)	$2 H_{2 (g)} + 4 O H_{(a q)}^{-} \to 4 H_{2} O_{(l)} + 4 e^{-}$	(iii)	Electrolysis of concentrated $H_{2} S O_{4}$
(D)	$2 F e_{(s)} + O_{2 (g)} + 4 H_{(a q)}^{+} \to 2 F e_{(a q)}^{2 +} + 2 H_{2} O_{(l)}$	(iv)	Reaction at anode in fuel cell

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