Ecell =0 or G =0 this condition is applicable on :
1. Spontaneous reaction
2. Equilibrium reaction
3. Non-Equilibrium reaction
4. None of the above
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. \(2.12 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}}\)
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?
1. 1.82 g
2. 1.95 g
3. 2.01 g
4. 1.16 g
E0cell for non-feasible type cell reaction is :
1. \(E_{cell}^{\circ }\) = Positive
2. \(E_{cell}^{\circ }\)= Negative
3. \(E_{cell}^{\circ }\) = Zero
4. None of the above.
E0cell for feasible type cell reaction is :
1.E0cell = 0
2. E0cell > 0
3. E0cell < 0
4. None of the above.
Absolute electrode potential of an electrode can't be measured because :
1. Oxidation or reduction can not occur alone.
2. Oxidation or reduction can occur alone.
3. Absolute electrode potential is intensive property.
4. Absolute electrode potential is extensive property.