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. \(2.12 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}}\)
The resistance of a cell containing 0.001 M KCl solution at 298 K is 1500 Ω. The conductivity is 0.146 × 10–3 S cm–1. The cell constant would be-
1. | 2. | ||
3. | 4. |
The amount of charge required for the reduction of 1 mol of to is -
The number of Faradays required to produce 20.0 g of Ca from molten CaCl2 is-
1. 2F
2. 1F
3. 4F
4. 3F
Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3, and CuSO4, respectively are connected in series.
A steady current of 1.5 amperes was passed through them until 1.45 g of silver was deposited at the cathode of cell B. The current flow time is-
1. 14 minutes
2. 25 minutes
3. 20 minutes
4. 11 minutes
The cell in which the following reactions occurs:
has \(E_{cell}^{o}\) = 0.236 V at 298 K.
The equilibrium constant of the cell reaction is :