Q. No.The potential of hydrogen electrode in contact with a solution with pH =10, is:
1.
−0.0591 V
2.
−5.91 V
3.
0.0591 V
4.
−0.591 V
| 1. | Cu & Zn2+ | 2. | Zn & Cu |
| 3. | Cu2+ & Zn2+ | 4. | Cu2+ & Zn |
| 1. | Increases | 2. | Decreases |
| 3. | Unchanged | 4. | Can't be predicted |
\(\wedge=\wedge_{0}-A \sqrt{C}\)
Which of the following equality holds?
\(\text { 1. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \sqrt{\Lambda}\)
\(\text { 2. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \infty\)
\(\text { 3. } \Lambda=\Lambda_{0} \text { as } \mathrm{C} \longrightarrow 0\)
\(\text { 4. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow 1\)
(Atomic weight of copper = 63.5)
1. 1 F
2. 2 F
3. 3 F
4. 4 F
| a. | It is also known as the Leclanche cell. |
| b. | The electrolyte is a moist paste of ammonium chloride (NH4Cl) and zinc chloride (ZnCl2). |
| c. | The cathodic reaction is : MnO2 + NH4++ e-→ MnO(OH) + NH3 |
| 1. | Only a and b are correct | 2. | Only c is correct |
| 3. | Only b and c are correct | 4. | All are correct |
1. \(0.1 Sm^{-1}\)
2. \(1 Sm^{-1}\)
3. \(10~ S~m^{-1}\)
4. \(4 \times 10^{-4} S~m^{-1}\)
\(\land^o_m\) for NaCl, HCl and \(\mathrm{CH_3COONa }\) are 126.4, 425.9, and 91.05 S cm2 mol–1 respectively. If the conductivity of 0.001028 mol L–1 acetic acid solution is \(4.95 \times 10^{-5} S ~cm^{-1} \), the degree of dissociation of the acetic acid solution is:
1. 0.01233
2. 1.00
3. 0.1233
4. 1.233
Aluminium oxide may be electrolysed at 1000 °C to furnish aluminium metal.
The cathode reaction is Al3+ + 3e- → Al.
To prepare 5.12 kg of aluminium metal by this method would require:
(Atomic mass = 27 amu; 1 faraday=96,500 Coulombs)
1. 5.49×101 C of electricity
2. 5.49×104 C of electricity
3. 1.83×107 C of electricity
4. 5.49×107 C of electricity
Two half cell reactions are given below:
\(\begin{aligned} &\mathrm{{Co}^{3+}+e^{-} \rightarrow {Co}^{2+}, {E}_{{Co}^{2+} / {Co}^{3+}}^{\circ}=-1.81 {~V}} \\ &2 \mathrm{{Al}^{3+}+6 e^{-} \rightarrow 2 {Al}({s}), {E}_{{Al} / {Al}^{3+}}^{\circ}=+1.66 {~V}} \end{aligned} \)
The standard EMF of a cell with feasible redox reaction will be:
| 1. | +7.09 V | 2. | +0.15 V |
| 3. | +3.47 V | 4. | –3.47 V |
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