Electrolysis

Step 1: Understand the Given Information:
The problem states that a current of 15.0 amperes is passed through a solution of CrCl2 for 45 minutes. The volume of Cl2 obtained at the anode at 1 atm and 273 K is to be calculated. The constants provided are:
, atomic weight of Cl = 35.5, and .

Step 2: Use Faraday’s Law of Electrolysis:
We can apply Faraday’s law to calculate the volume of Cl2 gas produced. Faraday’s law states that the amount of substance liberated or deposited at an electrode is directly proportional to the quantity of charge passed:

where:
- A (current)
- (time)
- (the number of moles of electrons involved in the half-reaction of Cl2)
- L·atm·mol^-1K^-1 (gas constant)
- K (temperature)
- atm (pressure)

Step 3: Calculate the total charge passed:
The total charge passed is given by:

Step 4: Apply Faraday's Law to Calculate Volume:
The volume of Cl2 produced is calculated as:

Final Answer:
The volume of Cl2 produced is 4.7 L.

Step 1: Analyzing Each Statement
1. Statement (i): Incorrect. Carbon tetrachloride ( ) does not undergo hydrolysis easily because it lacks vacant -orbitals, making it resistant to nucleophilic attack by water molecules. 2. Statement (ii): Correct. Diamond has a tetrahedral structure where each carbon atom is bonded to four other carbon atoms through strong directional covalent bonds, giving it high hardness and rigidity. 3. Statement (iii): Incorrect. Graphite, not fullerene, is the most thermodynamically stable allotrope of carbon due to its lower energy configuration. 4. Statement (iv): Correct. Glass is an amorphous, man-made silicate composed mainly of silica ( ), which is fused with other compounds like sodium oxide and calcium oxide.

Step 2: Evaluating the Given Options
- Option (1): Incorrect, as a statement (i) is incorrect.
- Option (2): Correct, as statements (ii) and (iv) are the only correct ones.
- Option (3): Incorrect, as a statement (iii) is incorrect.
- Option (4): Incorrect, as a statement (i) is incorrect.
Thus, the correct answer is

Option (2).

Step 1: Understanding Standard Electrode Potential
The standard electrode potential ( ) of an element is a measure of the tendency of the element to gain or lose electrons in an electrochemical reaction. It is given in volts ( ) and is measured under standard conditions.

Step 2: Standard Electrode Potentials for Lithium and Sodium
- For lithium, the standard reduction potential is: - For sodium, the standard reduction potential is:

Step 3: Evaluating the Given Options
- Option (1): Correct as per standard data.
- Option (2): Incorrect as the values are reversed.
- Option (3): Incorrect as the value for sodium is wrong.
- Option (4): Incorrect as the value for lithium is wrong.
Thus, the correct answer is

Option (1).

Step 1: Understanding Electrolysis of Molten NaCl
- When molten sodium chloride ( ) is electrolysed using platinum electrodes, it undergoes the following reactions:
- At the cathode ( ): (Sodium metal is deposited)
- At the anode ( ): (Chlorine gas is liberated)
- Therefore, Statement I is correct since is indeed liberated at the anode.
Step 2: Understanding Electrolysis of Aqueous CuSO
- When aqueous copper sulfate ( ) is electrolysed using platinum electrodes:
- At the cathode: (Copper is deposited)
- At the anode: (Oxygen gas is liberated)
- However, the oxygen gas is liberated at the anode, not at the cathode, making Statement II incorrect.
Step 3: Evaluating the Given Options
- Option (1): Incorrect, because Statement II is incorrect.
- Option (2): Incorrect, as Statement I is correct.
- Option (3): Correct, as Statement I is correct, and Statement II is incorrect.
- Option (4): Incorrect, as Statement I is correct.
Thus, the correct answer is

Option (3).