Pairs of reactants (R) and product (P) are given below. The pair which can be used in a fuel cell is :
1.
2.
3.
4.
The negative sign in the expression EoZn2+/Zn = -0.76 V indicates :
1. Metal reactivity increases.
2. Metal reactivity decreases.
3. No effect on metal.
4. None of the above.
Electrode potential is the potential difference between the -
1. Electrode and the electrolyte.
2. Anode and Cathode.
3. Anode and Atmosphere.
4. Cathode and Atmosphere.
1. | pH of the solution will rise. | 2. | pH of the solution will fall. |
3. | No change in the pH of the solution. | 4. | None of the above. |
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
The conductivity of 0.00241 M acetic acid is 7.896 × 10–5 S cm–1. If for acetic acid is 390.5 S cm2 mol–1, the dissociation constant will be
1. \(2.45 \times 10^{-5} \mathrm{~mol} \ \mathrm{~L}^{-1} \)
2. \(1.86 \times 10^{-5} \mathrm{~mol} \ \mathrm{L^{-1}} \)
3. \(3.72 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}} \)
4. \(2.12 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}}\)
One liter of 0.5 M KCl solution is electrolyzed for one minute in a current of 1.608 mA. Considering 100 % efficiency, the pH of the resulting solution will be :
1. | 7 | 2. | 9 |
3. | 8 | 4. | 10 |
Molten sodium chloride conducts electricity due to the presence of:
1. Free ions.
2. Free molecules.
3. Free electrons.
4. Atoms of sodium and chlorine.
At , the standard emf of a cell reaction involving a two-electron exchange is found to be 0.295 V. The equilibrium constant of the reaction is approximately :
1.
2.
3. 10
4.
For the electrolysis of CuSO4 solution the correct option is:
1. Cathode reaction: Cu2+ + 2e- Cu using Cu electrode.
2. Anode reaction: Cu Cu+ + e- using Cu electrode.
3. Cathode reaction: 2H+ + 2e- H2 using Pt electrode.
4. Anode reaction: Cu Cu2+ + 2e- using Pt electrode.