Advertisements
Advertisements
प्रश्न
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
Advertisements
उत्तर
\[\ce{\underset{(1 mol)}{Cu^{2+}} + \underset{(2 mol)}{2e^-} -> Cu}\]
∴ Required charge = 2 Faradays
= 2 × 96500 C
= 1.93 × 105 C
= 193000 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?
Consider the reaction: \[\ce{Cr2O^{2-}_7 + 14H^+ + 6e^- -> 2Cr^{3+} + 7H2O}\]
What is the quantity of electricity in coulombs needed to reduce 1 mol of \[\ce{Cr2O^{2-}_7}\]?
How much charge is required for the following reduction:
1 mol of Al3+ to Al?
How much charge is required for the following reduction:
1 mol of \[\ce{MnO^-_4}\] to Mn2+?
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?
On passing 1.5 F charge, the number of moles of aluminium deposited at cathode are _______ [Molar mass of Al = 27 gram mol–1]
(A) 1.0
(B) 13.5
(C) 0.50
(D) 0.75
What is the ratio of volumes of H2 and O2 liberated during electrolysis of acidified water?
(A) 1 : 2
(B) 2 : 1
(C) 1 : 8
(D) 8 : 1
Explain Faraday’s second law of electrolysis
Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.
How many faradays of electricity are required to produce 13 gram of aluminium from aluminium chloride solution? (Given: Molar mass of Al = 27.0-gram mol–1)
Electrolytic cell uses electrical energy to bring about ____________.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.
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 ______.
On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.
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).
On passing electricity through nitrobenzene solution, it is converted into azobenzene. The mass of azobenzene is ______ mg, if the same quantity of electricity produces oxygen just sufficient to burn 96 mg of fullerene (C60)·
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:
