Match list I with list II.
List I List II
A) Electrolysis of aq. $N a_{2} S O_{4}$ using Pt electrodes
1) 1 Faraday
B) The charge carried by $6.023 \times 10^{23}$ electrons is 2) 3 Faradays
C) The amount of electricity required to deposit 27 grams of Aluminium at cathode from molten $A l_{2} O_{3}$ is 3) $H_{2 (g)} /$ Pt
D) A gas in contact with an inert electrode 4) $O_{2}$ at anode $H_{2}$ at cathode

A-2, B-3, C-4, D-1

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A-4, B-1, C- 2, D-3

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A-3, B-2, C-4, D-1

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A-4, B-3, C-2, D-1

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Solution

The correct option is B A-4, B-1, C- 2, D-3

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A, B, C, D

^{'} n^{'}

P V^{n} = const

\begin{matrix} List I & List II A . & A & 1. & 0 B & B & 2 & 1 C & C & 3. & 1.4 D & D & 4. & \infty \end{matrix}

List-I	List-II
A. Mond’s process	1. Purification of Ag containing Pb
B. Van Arkel method	2. Purification of Ge
C. Cupellation	3. Purification of Nickel
D. Zone refining	4. Purification of Titanium

\begin{matrix} List - I & List - II (Metals) & (Extraction Process) (a) A u & (1) Self reduction (b) A l & (2) Liquation (c) P b & (3) Electrolysis (d) S n & (4) Bayer process \end{matrix}

Match List I with List II and select the correct answer using the codes given below the lists

List I (Compound) List II (Oxidation state of N)

(A) $N O_{2}$ (1) +5

(B) $H N O$ (2) -3

(D) $N_{2} O_{5}$ (4) +1

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A) Electrolysis of aq. $N a_{2} S O_{4}$ using Pt electrodes	1) 1 Faraday
B) The charge carried by $6.023 \times 10^{23}$ electrons is	2) 3 Faradays
C) The amount of electricity required to deposit 27 grams of Aluminium at cathode from molten $A l_{2} O_{3}$ is	3) $H_{2 (g)} /$ Pt
D) A gas in contact with an inert electrode	4) $O_{2}$ at anode $H_{2}$ at cathode