How much chlorine will be liberated on passing one ampere current for 30 min. through NaCl solution ?

• 0.66 mole

• 0.33 mole

• 0.66 g

• 0.33 g

Three ampere currernt was passed through an aqueous solution of an unknown salt of Pd for 1 h 2.977 g of Pdⁿ⁺ was deposited at cathode.The value of n is:

(given at wf of Pd= 106.4)

• 6

• 5

• 4

• 3

The metal which can displace all other metals from their salt solution among the following is:

• Al

• Zn

• Cu

• Fe

The standard reduction potentials of half reactions are given below:

F₂ (g) + 2e^- $\to$ 2F^- (aq) ; E⁰ = + 2.85 V

Cl₂ (g) + 2e^- $\to$2Cl^- (aq) ; E⁰ = + 1.36 V

Br₂ (g) + 2e^- $\to$2Br^- (aq) ; E⁰ = + 1.06 V

I₂ (g) + 2e^- $\to$ 2I^- (aq) ; E⁰ = + 0.53 V

The strongest oxidising and reducing agents respectively are:

• chlorine and iodine

• fluorine and iodine ion

• chloride and bromine

• bromine and iodine

Equivalent conductance of O .0128 N acetic acid solution, at 25°C is 14 ohm^-1 eq^-1 and at infinite dilution is 391 ohm-1eq^-1 .The degree of dissociation of acetic acid in the solution and its dissociation constant, respectively are:

• 0.036 and 1.66x10^-5

• 0.121 and 1.78x10^-4

• 0 .213 and 1.84x10^-5

• O .054 and 1.94x10^-4

Two metals 'A' and 'B' have E${}_{\mathrm{red}}^{°}$, value equal to 0.36 V and 1.23 V. What will be the correct cell equation?

• A + B²⁺ $\to$ A²⁺ + B

• A²⁺ + B $\to$ A + B²⁺

• Both (a) and (b)

• None of the above

Ag | AgCl | Cl^- (C₂) || Cl^- (C₁) | AgCl | Ag for this cell $∆$G is negative if:

• C₁ = C₂

• C₁ > C₂

• C₂ > C₁

• both (a) and (b)

Rusting of iron is a chemical reaction. The reaction is :

• double decomposition

• combination

• displacement

• analysis

Which one of the following conditions will increase the voltage of the cell represents by the equation?

Cu (s) + 2Ag⁺ (aq) $\to$ Cu²⁺ (aq) + Ag (s)

• Increase in the concentration of Ag⁺ ions

• Increase in the concentration of Cu²⁺ ions

• Increase in the dimensions of silver electrode

• Increase in the dimensions of copper electrode

650.

During the electrolysis of the aqueous solution of copper sulphate using Pt electrodes , the reaction taking place at the anode is:

• Cu²⁺ + 2e^- $\to$ Cu

• Cu $\to$ Cu²⁺ + 2e^-

• 2H₂O $\to$ 4H⁺ + O₂ + 4e^-

• H₂O + e^- $\to$ OH^- + $\frac{1}{2}$H₂