In the following reaction Pb undergoes- Pbs - PbO2s - 2H2SO4aq - 2 PbSO4s - 2H2Ol

The correct option is D comproportionationIn the reaction Pb changes to Pb^2+ and #160; Pb^4+ changes to #160; Pb^2+ . This is called ...

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Types of Redox Reactions

In the follow...

Question

In the following reaction $P b$ undergoes:
$P b (s)$ + $P b O_{2} (s)$ + $2 H_{2} S O_{4} (a q)$ $\to$ $2 P b S O_{4} (s)$ + $2 H_{2} O (l)$

disproportionation

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comproportionation

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reduction

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oxidation

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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)}

Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions:

(a) 2AgBr (s) + C₆H₆O₂(aq) → 2Ag(s) + 2HBr (aq) + C₆H₄O₂(aq)

(b) HCHO(l) + 2[Ag (NH₃)₂]⁺(aq) + 3OH^–(aq) → 2Ag(s) + HCOO^–(aq) + 4NH₃(aq) + 2H₂O(l)

(d) N₂H₄(l) + 2H₂O₂(l) → N₂(g) + 4H₂O(l)

(e) Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(s) + 2H₂O(l)

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

1.25 A

H_{2} S O_{4}

During discharging of lead-storage acid battery following reaction takes place:

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

If 2.5 amp of current is drawn for 965 minutes, $H_{2} S O_{4}$ consumed is:

(25^{\circ} C

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}

H_{2} S O_{4}

P b S O_{4 (s)}

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)

\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}

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