Advertisements
Advertisements
Question
Write any four applications of electrochemical series
Solution
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
APPEARS IN
RELATED QUESTIONS
96500 coulombs correspond to the charge on how many electrons?
How much electricity in terms of Faraday is required to produce 20 g of \[\ce{Ca}\] from molten \[\ce{CaCl2}\]?
(Given: Molar mass of Calcium is 40 g mol−1.)
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?
Suggest a list of metals that are extracted electrolytically.
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 \[\ce{Al^{3+}}\] to \[\ce{Al}\]?
How much charge is required for the following reduction:
1 mol of \[\ce{MnO^-_4}\] to \[\ce{Mn^{2+}}\]?
A solution of \[\ce{Ni(NO3)2}\] is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of \[\ce{Ni}\] is deposited at the cathode?
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 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)
Following reactions occur at cathode during the electrolysis of aqueous copper(II) chloride solution :
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why ?
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 )
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.
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?
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
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).
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:
