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Q. No.What is the nearest integer value of \(x\) for the Gibbs free energy change at 298 K, expressed as \(x×10^{−1}~kJ mol^{−1}\) for the given reaction.
\(Cu(s)+Sn^{2+}(0.001 M)\rightarrow Cu^{2+}(0.01M)+Sn(s) \)
Given: \(\small{E^\ominus_{Cu^{2+}/Cu}=0.34~V;~E^\ominus_{Sn^{2+}/Sn}=-0.14~V;~F=96500~C~mol^{-1}}\)
1. 873
2. 983
3. 1002
4. 911
\(Cu(s)+Sn^{2+}(0.001 M)\rightarrow Cu^{2+}(0.01M)+Sn(s) \)
Given: \(\small{E^\ominus_{Cu^{2+}/Cu}=0.34~V;~E^\ominus_{Sn^{2+}/Sn}=-0.14~V;~F=96500~C~mol^{-1}}\)
1. 873
2. 983
3. 1002
4. 911
Subtopic: Relation between Emf, G, Kc & pH |
56%
Level 3: 35%-60%
JEE
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Given below are two statements:
| Assertion (A): | Molar conductivity increases with a decrease in concentration. |
| Reason (R): | For strong electrolytes, \(Λ_m\) increases slowly with dilution and can be represented by the equation: \(\Lambda_m=\Lambda_m^0-A c^{1 / 2}\) |
| 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. | Both (A) and (R) are False. |
Subtopic: Conductance & Conductivity |
51%
Level 3: 35%-60%
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The Incorrect statement about the conductivity of electrolytic (ionic) solutions is:
| 1. | It is independent of the solvent viscosity |
| 2. | It depends on the size of the ions and their solvation |
| 3. | It increases with the increase in electrolyte concentration |
| 4. | It increases with the increase in temperature |
Subtopic: Conductance & Conductivity |
62%
Level 2: 60%+
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Subtopic: Electrode & Electrode Potential |
57%
Level 3: 35%-60%
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Extraction of chlorine from brine occurs when:
| 1. | \(\Delta G_V\) for the overall reaction is negative and EV for overall reaction has negative value. |
| 2. | \(\Delta G_V\) for the overall reaction is positive and EV for overall reaction has negative value. |
| 3. | \(\Delta G_V\) for the overall reaction is positive and EV for overall reaction has positive value. |
| 4. | \(\Delta G_V\) for the overall reaction is negative and EV for overall reaction has positive value. |
Subtopic: Relation between Emf, G, Kc & pH |
72%
Level 2: 60%+
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Consider the given two statements:
| Assertion(A): | \(\mathrm{E^0_{cell}}\) = 0 for a chloride ion concentration cell. |
| Reason(R): | For this concentration cell, the equation is given by: \(E_{\mathrm{cell}}=\frac{R T}{n F} \ln \left(\frac{\left[\mathrm{Cl}^{-}\right]_{\mathrm{LHS}}}{\left[\mathrm{Cl}^{-}\right]_{\mathrm{RHS}}}\right) \) |
| 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. |
Subtopic: Nernst Equation |
Level 3: 35%-60%
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Given below are some reactions. The reaction which is not feasible is
1. \(2KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2 \uparrow\)
2. \(2KCl + I_2 \rightarrow 2KI + Cl_2 \uparrow\)
3. Both 1 and 2 are not feasible
4. \(2KI + Cl_2 \rightarrow 2KCl + I_2\)
1. \(2KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2 \uparrow\)
2. \(2KCl + I_2 \rightarrow 2KI + Cl_2 \uparrow\)
3. Both 1 and 2 are not feasible
4. \(2KI + Cl_2 \rightarrow 2KCl + I_2\)
Subtopic: Electrochemical Series | Electrode & Electrode Potential |
Level 4: Below 35%
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When 50% \(H_2SO_4\) solution is electrolysed using inert electrodes, the products formed at anode and cathode, respectively, are
1. \(H_2 ~and ~O_2\)
2. \(O_2 ~and~H_2O_2\)
3. \(H_2O_2 ~and~ H_2\)
4. \(O_2 ~and ~H_2\)
1. \(H_2 ~and ~O_2\)
2. \(O_2 ~and~H_2O_2\)
3. \(H_2O_2 ~and~ H_2\)
4. \(O_2 ~and ~H_2\)
Subtopic: Electrolytic & Electrochemical Cell |
Level 4: Below 35%
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When \(CuSO_4\) solution using copper electrodes is electrolysed, pH of the solution
1. Increases
2. Decreases
3. Remains the same
4. Firstly increases and then decreases
1. Increases
2. Decreases
3. Remains the same
4. Firstly increases and then decreases
Subtopic: Faraday’s Law of Electrolysis |
Level 3: 35%-60%
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The feasible reaction, amongst the following, is
1. \(2KCl + Br_2 \rightarrow 2KBr + Cl_2\)
2. \(2KF + I_2 \rightarrow 2KI + F_2\)
3. \(2 KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2\)
4. \(2KIO_3 + Cl_2 \rightarrow 2KClO_3 + I_2\)
1. \(2KCl + Br_2 \rightarrow 2KBr + Cl_2\)
2. \(2KF + I_2 \rightarrow 2KI + F_2\)
3. \(2 KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2\)
4. \(2KIO_3 + Cl_2 \rightarrow 2KClO_3 + I_2\)
Subtopic: Electrochemical Series |
Level 3: 35%-60%
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