Use the data given above to find out the most stable ion in its reduced form.
1. | Cl- | 2. | Cr3+ |
3. | Cr | 4. | Mn2+ |
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+ |
The quantity of charge required to obtain one mole of aluminium from Al2O3 is :
1. 1 F
2. 6 F
3. 3 F
4. 2 F
The cell constant of a conductivity cell-
1. | Changes with the change of electrolyte. |
2. | Changes with the change of concentration of electrolyte. |
3. | Changes with the temperature of the electrolyte. |
4. | Remains constant for a cell. |
1. | PbSO4 anode is reduced to Pb. |
2. | PbSO4 cathode is reduced to Pb. |
3. | PbSO4 cathode is oxidised to Pb. |
4. | PbSO4 anode is oxidised to PbO2. |
\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -
1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)
The half-cell reaction at the anode during the electrolysis of aqueous sodium chloride solution is represented by :
1. Na+(aq) + e- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V \)
2. 2H2O(l) ⟶ O2(g) + 4H+(aq) + 4e- ; \(E_{cell}^{o} \) = 1.23 V
3. H+(aq) + e- ⟶ \(\frac{1}{2}\)H2(g) ; \(E_{cell}^{o} \) = 0.00 V
4. Cl-(aq) ⟶ \(\frac{1}{2}\)Cl2(g) + e- ; \(E_{cell}^{o}\)
The positive value of the standard electrode potential of Cu2+ / Cu indicates that-
(a) | This redox couple is a stronger reducing agent than the H+ /H2 couple |
(b) | This redox couple is a stronger oxidising agent than H+ /H2 |
(c) | Cu can displace H2 from acid. |
(d) | Cu cannot displace H2 from acid. |
of some half cell reactions are given below.
I: \(\mathrm{H}^{+} (a q)+e^{-} \rightarrow \frac{1}{2} \mathrm{H}_2 (g )\quad ; \quad E_{\text {cell }}^0=0.00 \mathrm{~V} \)
II: \(2 \mathrm{H}_2 \mathrm{O(l)} \rightarrow O_2 (g)+4 \mathrm{H}^{+} (a q)+4 e^{-} ; E_{\text {cell }}^{0}=1.23 \mathrm{~V} \)
III: \(2 \mathrm{SO}_4^{2-} (a q) \rightarrow \mathrm{S}_2 \mathrm{O}_8^{2-} (a q)+2 e^{-}, E_{\text {cell }}^{0}=1.96 \mathrm{~V} \)
The correct statements among the following are:
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 a dilute sulphuric acid solution, water will be oxidised at anode. |
d. | In dilute sulphuric acid solution, SO42- ion will be oxidised to tetrathionate ion at anode. |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, c)
= 1.1 V for Daniel cell. Which of the following expressions are correct descriptions of the state of equilibrium in this cell?
(a) 1.1 = KC
(b)
(c)
(d) log KC = 1.1
The correct choice among the given is -
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)