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:

\(Fe^{2+}(aq) \ + \ Ag^{+}(aq) \ \rightarrow \ Fe^{3+}(aq) \ + \ Ag(s)\)

\(E_{Fe^{3+}/Fe^{2+}}^{o} \ = \ 0.77 \ V; \ E_{Ag^{+}/Ag}^{o} \ = \ 0.80 \ V\)

The value of \(\Delta G_{r}^{o} \)  in the above reaction will be:

1. +$2.89$ $\mathrm{kJ}$

2. $-2.89$ $\mathrm{kJ}$

3. $-2.89$ $\mathrm{J}$

4. -186.83 J

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 coulombs of charge required for the oxidation of 1 mole of ${\mathrm{H}}_2{\mathrm{O}}_2$ to ${\mathrm{O}}_2$ is: 

1. $9.65\times {10}^4$ $\mathrm{C}$

2. 93000 C

3. $1.93\times {10}^5$ $\mathrm{C}$

4. $19.3\times {10}^2$ $\mathrm{C}$

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 : 

 2Cr(s) + 3Cd²⁺(aq) → 2Cr³⁺(aq) + 3Cd

${{\mathrm{E}}^{⊝}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}=$ $-0.74$ $\mathrm{V}$; ${{\mathrm{E}}^{⊝}}_{{\mathrm{Cd}}^{2+}/\mathrm{Cd}}=-0.40$ $\mathrm{V}$

The value of $∆{\mathrm{G}}_r^{\mathrm{o}}$ in the above reaction will be-