Q. No.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
Find the dissociation constant (Kₐ) of 0.00241 M acetic acid if its conductivity is 7.896 × 10⁻⁵ S cm⁻¹
and its molar conductivity at infinite dilution (Λₘ°) is 390.5 S cm² mol⁻¹.
2. 1.86 × 10⁻⁵ mol L⁻¹
3. 3.72 × 10⁻⁵ mol L⁻¹
4. 2.12 × 10⁻⁵ mol 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 nickel(Ni) is deposited at the cathode?
(Given Molar Mass of Ni = 58.7g)
| 1. | 1.82 g
|
2. | 2.95 g
|
| 3. | 7.01 g
|
4. | 5.16 g |
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 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 the cell B. The current flow time is:
1. 14 minutes
2. 25 minutes
3. 20 minutes
4. 11 minutes
Find the number of electrons that flow through a metallic wire when a current of 0.5 A passes through it for 2 hours.
1. 2.25 × 10²²2. 2.25 × 10⁻²²
3. 1.34 × 10²¹
4. 3.16 × 10²⁴
What is the quantity of electricity in coulombs needed to reduce 1 mol of ?
For the reaction:
1. 578992 C
2. 289461 C
3. 192974 C
4. 96487 C
What is the potential of hydrogen electrode in contact with a solution whose pH is 10?
1. 0.591 V
2. -0.591 V
3. 0.295 V
4. -0.295 V
What will be the emf of the cell in which the following reaction takes place? Given
1. 0.80 V
2. 0.91 V
3. 0.45 V
4. 0.36 V
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