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16
MCQ (Single Correct Answer)

$\Lambda_{\mathrm{m}\left(\mathrm{NH}_4 \mathrm{OH}\right)}^{\circ}$ is equal to ................ .

A
$\Lambda_{m\left(\mathrm{NH}_4 \mathrm{OH}\right)}^{\circ}+\Lambda_{m\left(\mathrm{NH}_4 \mathrm{Cl}\right)}^{\circ}-\Lambda_{(\mathrm{HCl})}^{\circ}$
B
$\Lambda_{m\left(\mathrm{NH}_4 \mathrm{Cl}\right)}^{\circ}+\Lambda_{m(\mathrm{NaOH})}^{\circ}-\Lambda_{(\mathrm{NaCl})}^{\circ}$
C
$\Lambda_{m\left(\mathrm{NH}_4 \mathrm{Cl}\right)}^{\circ}+\Lambda_{m(\mathrm{NaCl})}^{\circ}-\Lambda_{(\mathrm{NaOH})}^{\circ}$
D
$\Lambda_{m(\mathrm{NaOH})}^{\circ}+\Lambda_{m(\mathrm{NaCl})}^{\circ}-\Lambda_{\left(\mathrm{NH}_4 \mathrm{Cl}\right)}^{\circ}$
17
MCQ (Single Correct Answer)

In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?

A
$\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Na}(\mathrm{s}) E_{\mathrm{cell}}^{\mathrm{s}}=-2.71 \mathrm{~V}$
B
$2 \mathrm{H}_2 \mathrm{O}(\mathrm{I}) \longrightarrow \mathrm{O}_2(\mathrm{~g})+4 \mathrm{H}^{+}(\mathrm{aq})+4 \mathrm{e}^{-} E_{\text {cell }}^{\mathrm{s}}-1.23 \mathrm{~V}$
C
$\mathrm{H}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \frac{1}{2} \mathrm{H}_2(\mathrm{~g}) ; E_{\text {cell }}^{-}=0.00 \mathrm{~V}$
D
$\mathrm{Cl}^{-}(a q) \longrightarrow \frac{1}{2} \mathrm{Cl}_2(g)+e^{-} ; E_{\text {cell }}^{\mathrm{s}}=1.36 \mathrm{~V}$
18
MCQ (Multiple Correct Answer)

The positive value of the standard electrode potential of $\mathrm{Cu}^{2+} / \mathrm{Cu}$ indicates that ............ .

A
this redox couple is a stronger reducing agent than the $\mathrm{H}^{+} / \mathrm{H}_2$ couple
B
this redox couple is a stronger oxidising agent than $\mathrm{H}^{+} / \mathrm{H}_2$
C
Cu can displace $\mathrm{H}_2$ from acid
D
Cu cannot displace $\mathrm{H}_2$ from acid
19
MCQ (Multiple Correct Answer)

$\mathrm{E}_{\text {cell }}^{\mathrm{s}}$ for some half cell reactions are given below. On the basis of these mark the correct answer.

(a) $\mathrm{H}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \frac{1}{2} \mathrm{H}_2(\mathrm{~g})\qquad; \mathrm{E}_{\text {cell }}^{\mathrm{s}}=0.00 \mathrm{~V}$

(b) $2 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \longrightarrow \mathrm{O}_2(\mathrm{~g})+4 \mathrm{H}^{+}(\mathrm{aq})+4 \mathrm{e}^{-}\qquad$; $\mathrm{E}_{\text {cell }}^{\mathrm{s}}=1.23 \mathrm{~V}$

(c) $2 \mathrm{SO}_4^{2-}(\mathrm{aq}) \longrightarrow \mathrm{S}_2 \mathrm{O}_8^{2-}(\mathrm{aq})+2 \mathrm{e}^{-} ; \quad \mathrm{E}_{\text {cell }}^{\mathrm{s}}=1.96 \mathrm{~V}$

A
In dilute sulphuric acid solution, hydrogen will be reduced at cathode
B
In concentrated sulphuric acid solution, water will be oxidised at anode
C
In dilute sulphuric acid solution, water will be oxidised at anode
D
In dilute sulphuric acid solution, $\mathrm{SO}_4^{2-}$ ion will be oxidised to tetrathionate ion at anode
20
MCQ (Multiple Correct Answer)

$\mathrm{E}_{\text {cell }}^{\circ}=1.1 \mathrm{~V}$ or Daniel cell. Which of the following expressions are correct description of state of equilibrium in this cell?

A
$1.1=K_C$
B
$\frac{2.303 R T}{2 F} \log K_C=1.1$
C
$\log K_C=\frac{2.2}{0.059}$
D
$\log K_C=1.1$
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