The correct statement among the following options is:
1. | Ecell and ∆rG of cell reaction are both extensive properties. |
2. | Ecell and ∆rG of cell reaction are both intensive properties. |
3. | Ecell is an intensive property while ∆rG of cell reaction is an extensive property. |
4. | Ecell is an extensive property while ∆rG of cell reaction is an intensive property. |
The incorrect statement about the solution of electrolytes is:
1. | Conductivity of solution depends upon the size of ions. |
2. | Conductivity depends upon the viscosity of solution. |
3. | Conductivity does not depend upon the solvation of ions present in solution. |
4. | Conductivity of solution increases with temperature. |
The most stable oxidized species among the following is:
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)
1. | Cr3+ | 2. | MnO4- |
3. | Cr2O72- | 4. | Mn2+ |
Match Column-I (Types of cell) with Column-II (Characteristics shown by cells) and mark the appropriate option:
Column I (Type of cell) |
Column II (Characteristics) |
||
A | Lechlanche cell | 1. | Cell reaction 2H2 +O2 → 2H2O |
B | Ni-Cd cell | 2. | Does not involve any ion in solution and is used in hearing aids. |
C | Fuel cell | 3. | Rechargeable |
D | Mercury cell | 4. | -Reaction at anode, Zn → Zn2+ + 2e- |
Codes:
Options: | A | B | C | D |
1. | 2 | 3 | 4 | 1 |
2. | 4 | 3 | 1 | 2 |
3. | 1 | 4 | 3 | 2 |
4. | 4 | 1 | 3 | 2 |
Given below are two statements:
Assertion (A): | Cu is less reactive than hydrogen. |
Reason (R): | E°Cu2+/ Cu is negative. |
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. |
The electrode potential for Mg electrode varies according to the equation
\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\)
The graph of EMg2+ / Mg vs log [Mg2+] among the following is:
1. | 2. | ||
3. | 4. |
In a typical fuel cell, the reactants (R) and products (P) are:
1. | R = H2(g), O2(g); P = H2O2(l) |
2. | R = H2(g), O2(g); P = H2O(l) |
3. | R = H2(g), O2(g), C l2(g); P = HClO4(aq) |
4. | R = H2(g), N2(g); P = NH3(aq) |
The value of E0 cell for the following reaction is:
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ } \)
(Given, equilibrium constant is 106)
1. | 0.17 | 2. | 0.01 |
3. | 0.05 | 4. | 1.77 |
Consider the following reaction:
\(\frac{4}{3} \mathrm{Al}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \frac{2}{3} \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})\)
The minimum e.m.f. required to carry out the electrolysis of Al2O3 is:
(F = 96500 C mol–1)
1. 2.14 V
2. 4.28 V
3. 6.42 V
4. 8.56 V
Mg(s) + 2Ag+(0.0001M) → Mg2+(0.130M) + 2Ag(s)
If EƟ(cell) for the above mentioned cell is 3.17 V, then E(cell) value will be-
(log 13=1.1)
1. 2.87 V
2. 3.08 V
3. 2.96 V
4. 2.68 V