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1. Mark the correct Nernst equation representation for the following cell :
\(\mathrm{Fe}_{(s)}\left|\mathrm{Fe}^{2+}(0.001 \mathrm{M})\right|\left|\mathrm{H}^{+}(1 \mathrm{M})\right| \mathrm{H}_{2(g)}(1 \mathrm{bar}) \mid \mathrm{Pt}_{(s)}\)

1.	\( E_{\text {cell }}=E_{\text {cell }}^{\circ}-\frac{0.591}{2} \log \frac{\left[\mathrm{Fe}^{2+}\right]\left[\mathrm{H}^{+}\right]^2}{[\mathrm{Fe}]\left[\mathrm{H}_2\right]}\)
2.	\(E_{\text {cell }}=E_{\text {cell }}^{\circ}-\frac{0.591}{2} \log \frac{[\mathrm{Fe}]\left[\mathrm{H}^{+}\right]^2}{\left[\mathrm{Fe}^{2+}\right]\left[\mathrm{H}_2\right]} \)
3.	\(E_{\text {cell }}=E_{\text {cell }}^{\circ}-\frac{0.0591}{2} \log \frac{\left[\mathrm{Fe}^{2+}\right]\left[\mathrm{H}_2\right]}{[\mathrm{Fe}]\left[\mathrm{H}^{+}\right]^2} \)
4.	\(E_{\text {cell }}=E_{\text {cell }}^{\circ}-\frac{0.0591}{2} \log \frac{[\mathrm{Fe}]\left[\mathrm{H}_2\right]}{\left[\mathrm{Fe}^{2+}\right]\left[\mathrm{H}^{+}\right]^2}\)

2. The reaction: 
\(\frac{1}{2} \mathrm{H}_2(\mathrm{~g})+\mathrm{AgCl}(\mathrm{s}) \rightarrow \mathrm{H}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Ag}(\mathrm{s})\)
occurs in the galvanic cell. The correct cell representation is given by:
1. \(\small\mathrm{Ag}(s)\mid \mathrm{AgCl}(s)\mid \mathrm{KCl}(soln)\mid \mid\mathrm{AgNO}_3(soln) \mid \mathrm{Ag}(s)\)
2. \(\mathrm{Pt} \mid \mathrm{H}_2 (g) \mid \mathrm{HCl} (soln) \mid \mid\mathrm{AgNO}_3 (soln) \mid \mathrm{Ag}(s)\)
3. \(\mathrm{Pt} \mid \mathrm{H}_2 (g) \mid \mathrm{HCl} (soln) \mid\mid \mathrm{AgCl} (s) \mid \mathrm{Ag}(s)\)
4. \(\mathrm{Pt} \mid \mathrm{H}_2 (g) \mid \mathrm{KCl} (soln) \mid\mid \mathrm{AgCl} (s) \mid \mathrm{Ag}(s)\)  

3. Standard electrode potential for the cell with cell reaction
Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)
is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction. (Given F = 96487 C mol^–1)

1.	–200.27 kJ mol–1	2.	–212.27 kJ mol–1
3.	–212.27 J mol–1	4.	–200.27 J mol–1

4. The limiting molar conductivities of a divalent cation \(\left(\mathrm{M}^{2+}\right)~\)and a monovalent anion \(\left(\mathrm{A}^{-}\right)~\)are \(57 \mathrm{~S} \mathrm{~cm}^2\) \( \mathrm{mol}^{-1}\) and \(73 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\) respectively. What is the limiting molar conductivity of their compound in \(\mathrm{S}~ \mathrm{cm}^2 \mathrm{~mol}^{-1}\)?
1. 203 
2. 421
3. 143 
4. 303

5.

The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. The cell constant, if conductivity of 0.001 M KCl solution at 298 K is 0.146 ×10^-3  S cm^-1, will be: 
1. 0.32 cm^-1
2. 0.47 cm
3. 0.22 cm^-1
4. 0.23 cm

6. The time needed by a current of 4.00 amp applied to a solution of Cu²⁺(aq) to produce 2.0 grams of copper metal will be:
1. 2.4 × 10⁴ s
2. 1.5 × 10³ s
3. 7.6 × 10² s
4. 3.8 × 10² s

7. Consider the given two statements:

Statement I:	A Daniel cell consists of zinc and copper electrodes immersed in solutions of their respective salts.
Statement II:	Mercury cell consists of zinc–mercury amalgam as the anode and a paste of HgO & carbon as the cathode.

 

1.	Statement I is incorrect and Statement II is correct.
2.	Both Statement I and Statement II are correct.
3.	Both Statement I and Statement II are incorrect.
4.	Statement I is correct and Statement II is incorrect.

8.

Assertion (A):	The standard reduction potentials of three metallic ions A, B, and C are –0.3, –0.5, and 0.8 volts respectively. Therefore, the oxidizing power of ions is C > A > B.
Reason (R):	The higher the standard reduction potential, the higher the oxidizing power.

 

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	(A) is False but (R) is True.

9. 'Leclanche cell' is also known as:
1. Mercury Cell
2. Dry Cell
3. Lead cell
4. Nickel‐cadmium cell

10.

E⁰_cell for  non-feasible type cell reaction is :
1. \(E_{cell}^{\circ }\) = Positive
2. \(E_{cell}^{\circ }\)= Negative
3. \(E_{cell}^{\circ }\) = Zero
4. None of the above.