Application of Electrolysis
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Q.
As compared to lithium, sodium reacts quickly with water because
Its molecular weight is less
It is stronger electronegative
It is stronger electropositive
It is a metal
Q.
Aqueous solution of the following compound on electrolysis gives ethane
Potassium acetate
Ethyl acetate
Acetic acid
Acetamide
Q. Which of the following statements is/are true for the electrolysis of aq.LiCl with Ag electrodes?
Ag get dissolved to give Ag+ at anode
- Ag is deposited at cathode
- O2 is liberated at anode
- Cl2 is liberated at anode
Q. Calculate the reduction potential for the following half cell at 25∘C:
Ag(s)|Ag+(aq, 10−5 M); E0Ag+/Ag=−0.80 V
Ag(s)|Ag+(aq, 10−5 M); E0Ag+/Ag=−0.80 V
- EAg+/Ag=0.5 V
- EAg+/Ag=0.25 V
- EAg+/Ag=0.8 V
- EAg+/Ag=1.5 V
Q.
Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible.
Ag(s) and Fe3+(aq)Q. 100 mL of a 0.05 M CuSO4 aqueous solution was electrolysed using inert electrodes by passing current till the pH of the resulting solution was 2. The solution after electrolysis was neutralised and then treated with excess KI and the formed I2 was titrated with 0.04 M Na2S2O3. Calculate the volume of Na2S2O3 required in mL.
- 112.5 mL
- 100 mL
- 125 mL
- None of these
Q. Pt(s)∣M(s)∣M3+(aq, 0.002 mol L−1)∥Ag+(aq, 0.01 mol L−1)∣Ag(s)
The emf of the given cell is found to be 0.42 V at 25 ∘C. Calculate the standard reduction potential of the half reaction.
M3+(aq) + 3e−→M(s)
Given:E0Ag+/Ag = 0.80 V, log2=0.3
The emf of the given cell is found to be 0.42 V at 25 ∘C. Calculate the standard reduction potential of the half reaction.
M3+(aq) + 3e−→M(s)
Given:E0Ag+/Ag = 0.80 V, log2=0.3