What will happen during the electrolysis of an aqueous solution of CuSO₄ by using platinum electrodes?

The correct choice among the given is -

The number of Faradays (F) required to produce 20 g of calcium from molten CaCl₂ (Atomic mass of Ca = 40 g mol^–1) is:

1. 2

2. 3

3. 4

4. 1

The amount of charge required for the reduction of 1 mol of ${\mathrm{MnO}}_4^{-}$ to ${\mathrm{Mn}}^{2+}$ is -

$1.$ $4.8$ $\times$ ${10}^5$ $\mathrm{C}$
$2.$ $3.2$ $\times$ ${10}^6$ $\mathrm{C}$
$3.$ $1.8$ $\times$ ${10}^5$ $\mathrm{C}$
$4.$ $4.1$ $\times$ ${10}^4$ $\mathrm{C}$

The number of Faradays required to produce 20.0 g of Ca from molten CaCl₂ is-

1. 2F

2. 1F

3. 4F

4. 3F

The three cells with their \(E^\circ_{\text{(cell)}}\) values are given below:

What is the mass of copper deposited at the cathode after electrolyzing a solution of CuSO₄ for 10 minutes with a current of 1.5 amperes?

1. 0.36 g
2. 0.48 g
3. 0.30 g
4. 0. 22 g

The quantity of charge required to obtain one mole of aluminium from Al₂O₃ is :

1.  1 F

2.  6 F

3.  3 F

4.  2 F

The electricity required in coulombs for the oxidation of 1 mole of FeO to ${\mathrm{Fe}}_2{\mathrm{O}}_{\mathrm{3 }}$is: