Advertisements
Advertisements
प्रश्न
How much charge is required for the following reduction?
1 mol of \[\ce{MnO^-_4}\] to Mn2+.
Advertisements
उत्तर
The given reaction is:
\[\ce{\underset{(1 mol)}{MnO^-_4} + 8H^+ + \underset{(5 mol)}{5e^-} -> Mn^{2+} + 4H2O}\]
∴ 5 mole electrons are needed for the reduction of 1 mole of \[\ce{MnO^-_4}\] to Mn2+.
∴ 5 mole electrons = 5 Faradays
= 5 × 96500 C
= 4.825 × 105 C
APPEARS IN
संबंधित प्रश्न
96500 coulombs correspond to the charge on how many electrons?
If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?
Suggest a list of metals that are extracted electrolytically.
How much charge is required for the following reduction?
1 mol of Al3+ to Al.
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 deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?
Write any two uses of H2SO4
Draw neat labelled diagram of electrolytic refining of blister copper
State second law of electrolysis
Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO3 for 15 minutes.
(Given : Molar mass of Ag = 108 g mol−1 lF = 96500 C mol−1)
What will happen during the electrolysis of aqueous solution of \[\ce{CuSO4}\] by using platinum electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will deposit at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will dissolve at anode.
What will happen during the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will dissolve at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will deposit at anode.
Consider the figure and answer the following question.
Cell ‘A’ has ECell = 2V and Cell ‘B’ has ECell = 1.1V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?
When during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be ______.
The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.
A current of 4 amp was passed for 2 hours through a solution of copper sulphate when 5.0 g of copper was deposited. The current efficiency is ______% (Cu = 63.5).
Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.
Reason (R): The electrode potential of Cu2+/Cu is greater than that of H+/H2.
Select the most appropriate answer from the options given below:
How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?
(Given: Molar mass of Aluminium is 27 g mol−1.)
