The incorrect statement(s) among the below is/are:

(a)	The unit of conductivity is S cm–2
(b)	Specific Conductivity of weak and strong electrolytes always decreases with a decrease in concentration.
(c)	The unit of molar conductivity is S cm2 mol–1
(d)	Molar conductivity increases with an increase in concentration.

1. Only (a)

2. (a) and (d)

3. (b) and (d)

4. (a) and (c)

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm^–1. The molar conductivity will be -

The electricity required in coulombs for the oxidation of 1 mole of FeO to \(Fe_{2} O_{3 }\) is:

The value of E_cell in the reaction below will be:

\(\small{Pt(s)|Br^{-}(0.010 \ M)|Br_{2}(l) \ ||H^{+}(0.030 \ M)|H_{2}(g)(1 \ bar)|Pt(s)}\)

\(E_{Br^{-}/Br_{2}}^{o} \ = \ -1.09 \ V\)
1. +1.298 V

The value of  ∆G°  in the reaction below would be:
\(\small{\mathrm{Zn}(\mathrm{s})+\mathrm{Ag}_2 \mathrm{O}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{Zn}^{+2}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq})}\)

Given: \(E_{cell}^{\circ} = 1.04V\)

1. –2.13 kJ

2. –21.3 kJ

3. –201 kJ

4. –31.12 kJ

The mass of nickel deposited by electrolysis of a solution of $\mathrm{Ni}{\left({\mathrm{NO}}_3\right)}_2$ using a current of 5 amperes for 20 min is: 
(Atomic mass of Nickle is 58.7u)

1. 2.42 g

2. 1.82 g

3. 3.93 g

4. 6.42 g

Consider the following graph.

The strong electrolyte in the above graph is represented by:

1. X

2. Y

3. Both X and Y

4. Data given is not sufficient to predict.

Consider the following graph of molar conductivity of KCl solution at different concentrations. 

 

The value of limiting molar conductivity for KCl is 150.0 S cm² mol^-1. The value of the slope at point A will be : 

The molar conductance of NaCl, HCI, and CH₃COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol^–1 respectively. The molar conductance of CH₃COOH at infinite dilution will be:

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