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प्रश्न
Write any four applications of electrochemical series
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उत्तर
applications of electrochemical series :
1. Oxidizing and Reducing Strengths.
2. Comparison of Reactivities of Metals
3. Calculation of the EMF of the Cell
4. Predicting the Liberation of Hydrogen Gas from Acids by Metals
5. Predicting Feasibility of a Redox Reaction
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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
The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is -
- 2098
- 96500
- 193000
- 4196
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
Suggest a list of metals that are extracted electrolytically.
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
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?
Draw neat labelled diagram of electrolytic refining of blister copper
State second law of electrolysis
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.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur 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.
Assertion: Electrolysis of NaCl solution gives chlorine at anode instead of O2.
Reason: Formation of oxygen at anode requires overvoltage.
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 ______.
Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is
On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.
What is the quantity of electricity in Coulombs required to produce 4.8 g of Mg from molten MgCl2? How much Ca will be produced if the same amount of electricity was passed through molten CaCl2? (Atomic mass of Mg = 24 u, atomic mass of Ca = 40 u).
Through an aqueous solution of an unknown salt of metal M (M = 200 g/mol) a current of 1.93 A is passed for 50 min. If 4 g of metal is produced at cathode. The charge on metal ion in solution is ______.
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.)
