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- Definition of electrochemistry electrolysis
- Why the study of electrochemistry is important?
- Basic function of Galvanic cell/ voltaic cell
- How current flows in the electrolytic solution and name the species responsible for the same
- Nature of the anode sign (+/-) in a galvanic cell
- Daniell cell has an electrical potential equal to 1.1 V . Study the movement of electrons/ ions and the deposition of metal on their respective electrodes when (i)Eext = 1.1 V , (ii)Eext < 1.1 V and (iii)Eext > 1.1 V
- Concept of half cell / redox couple and when an electrode potential will said to be slandered electrode potential
- How anode and cathode get the +ve and –ve potential with respect to the solution
- Definition of cell potential its application in numerical
- Definition of electromotive force (emf)
- A good practice on writing the half cell balanced reaction and analyzing whether the reaction is of oxidation or reduction
- Significance of salt bridge
- Concept of standard hydrogen electrode and calculation of emf by using the formula
- How would you determine the standard electrode potential of the system Mg2+|Mg?
- A good analysis of electrochemical series interms of position of elements and their emf
- Significance of +ve and –ve Eo
- Good study about the preferential discharge theory
- Derivation of Nernst equation step by step and get a connectivity of formulae for the numerical purpose
- Nurnst equation for a chemical reaction
- Represent the cell in which the following reaction takes place
Mg(s) + 2Ag + (0.0001M) -----> Mg2+ (0.130M) + 2Ag(s)
Calculate its E(cell), if (cell) EV = 3.17 V.
- Relation of equilibrium constant with Nurnst equation
- Calculate the equilibrium constant of the reaction:
Cu(s) + 2Ag +(aq) -------> Cu2+(aq) + 2Ag(s)
E (cell) = 0.46 V
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- Concept and definition of Gibbs energy
- Relation between Gibbs energy with Nurnst equation
- Formula to calculate the standard Gibbs energy equilibrium constant
- Calculate the potential of hydrogen electrode in contact with a solution whose pH is 11.
- Write the whole equations for the electrolysis of the following and mention the species that are collected on anode and cathode
- CuSO4 by using Pt- Electrode
- Molten PbBr2 using Pt- Electrode
- AgNO3 by using Ag electrode
- What is the quantitative relationship between charge and deposited amount? Or describe the Faraday’s first law
- Definition of electrochemical equivalent (z). It depends on mass or not. It is an intensive property or not
- Define the faraday law for the gaseous electrolytic product
- Fined the weight of Cu deposited due to the electrolysis of CuSO4(aq)By passing 965 coulomb of charge
- Fined the amount of chlorine evolved at anode due to electrolysis of aq. NaCl by passing 965 coulomb of charge. And also fined the volume of hydrogen evolved
- Calculation of weight deposited at electrode when dimension of electrode is given
- What is current efficiency? Describe the formula for the same
- A current of 4 amp. Is passed for 1.5 Hr through a solution of CuSO4 and then 3.2 gm Cu is deposited .Fined the current efficiency
- Define the Faraday’s second law and how it is useful for the numerical
- Calculation of number of Faraday required to deposit one mole of substance at respective electrode or to oxidize/ reduce one mole of any substance
- What are the applications of electrolysis?
- Define electroplating with it aim
- How electrolysis is useful in purification of metals
- Define conductance and conductivity
- What is specific conductance or conductivity?
- What is the effect of dilution on specific conductivity?
- What is cell constant? Formula to calculate the cell constant
- Equivalent conductance and its unit
- Relation between molar conductance and equivalent conductance
- kohlrausch law or law of independent migration of ions and it application
- If the molar conductivity at infinite dilution of NaCl, HCl and CH3COONa are 126.6, 426.1 and 91.00 Ohm-1 Cm2 gm Eq-1. What will be the molar conductivity of CH3COOH
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