Advertisements
Advertisements
प्रश्न
Number of faradays of electricity required to liberate 12 g of hydrogen is:
पर्याय
1
8
12
16
Advertisements
उत्तर
12
- The molecular mass of Hydrogen is 1 gram and has a single electron in its configuration as it is the first most element of the periodic table.
- The 12 grams of Hydrogen contains 12 moles of the electrons in it. Usually, the electricity will be passed through the free electrons.
- The 12 grams of Hydrogen contains 12 electrons which are free electrons.
- Each free electron is capable of conducting 1 Faraday of electricity.
- Since 12 grams of Hydrogen are having 12 electrons in it, we require 12 Faraday of electricity.
APPEARS IN
संबंधित प्रश्न
On calculating the strength of current in amperes if a charge of 840C (coulomb) passes through an electrolyte in 7 minutes, it will be
- 1
- 2
- 3
- 4
96500 coulombs correspond to the charge on how many electrons?
How much electricity in terms of Faraday is required to produce 20 g of Ca from molten CaCl2?
(Given: Molar mass of Calcium is 40 g mol−1.)
Using the E° values of A and B, predict which is better for coating the surface of iron [E°(Fe+2/Fe) = -0.44V] to prevent corrosion and why?
Given: E° (A+2/A)=-2.37 V: E°(B+2/B)= -0.14V
Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution:
Na+(aq) + e− ⟶ Na (s) E0 = 2.71 V
H+(aq) + e− ⟶ `1/2` H2 (g) E0 = 0.00 V
On the basis of their standard reduction electrode potential (E0) values, which reaction is feasible at the cathode and why?
If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?
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?
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
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 much quantity of electricity in coulomb is required to deposit 1.346 × 10-3 kg of Ag in 3.5 minutes from AgNO3 solution?
( Given: Molar mass of Ag is 108 × 10-3 kg mol-1 )
Solve the following question.
A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO4 and ZnSO4 until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y.
(Molar mass : Fe = 56 g mol–1, Zn = 65.3 g mol–1, 1F = 96500 C mol–1)
According to Faraday’s First Law of Electrolysis, the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the ____________.
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.
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.
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?
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.
The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.
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)·
