Molten sodium chloride conducts electricity due to the presence of: 

1. Free ions.

2. Free molecules.

3. Free electrons.

4. Atoms of sodium and chlorine.

The unit of specific conductance is:

The $k=$ $4.95$ $\times$ ${10}^{-5}S$ $c{m}^{-1}$ for a 0.00099 M solution. The reciprocal of the degree of dissociation of acetic acid, if ${\wedge }_m^0$ for acetic acid is 400 S $c{m}^{2}mo{l}^{-1}$ will be:

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Given: Charge on electron = 1.60 × 10^–19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$

The molar conductivity of 0.007 M acetic acid is 20 S cm² mol^–1. The dissociation constant of acetic acid is :

(\(\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }\))
(\(\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}\))

1. $1.75\times {10}^{-5}$ mol L^–1 

2. $2.50\times {10}^{-5}$ mol L^–1 

3. $1.75\times {10}^{-4}$ mol L^–1 

4. $2.50\times {10}^{-4}$ mol L^–1 

What happens to the voltage in a galvanic cell when the salt bridge is removed?

1. The voltage drops to zero.
2. The voltage remains the same.
3. The voltage gradually increases.
4. The voltage rapidly increases.

The electrode potential for the Mg electrode varies according to the equation:

\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\) 

The graph of E_{Mg²⁺ / Mg} vs log [Mg²⁺] among the following is:

1.		2.
3.		4.

Find the relationship between E₁ and E₂ for the following Daniell cell:

Zn | ZnSO₄ (0.01 M) || CuSO₄ (1.0 M) | Cu

The emf of this cell is E₁.

If the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ is changed to 0.01 M, the emf becomes E₂.

Given:

RT/F = 0.059 V

1. E₁ = E₂

2. E₁ > E₂

3. E₁ < E₂

4. E₂ = 0 \(\neq\)E₁

Identify the reactants (R) and product (P) in a typical fuel cell.