Flashcards for NEET Chemistry - Electrochemistry

Flashcards for NEET Chemistry are designed to boost your NEET preparation. Find below flashcards for the chapter β€œElectrochemistry”. These flashcards are prepared as per the NEET syllabus. These are helpful for aspirants of NEET and other exams, during last-minute revision. It covers all the important points that are frequently asked in the exam. Check BYJU’S, for the full set of Flashcards and Study material for NEET Chemistry.

Download PDF of NEET Chemistry Flashcards for Electrochemistry

Name of the NEET Sub-section


Flashcards Helpful for



NEET Exams

flashcards for neet chemistry dec13 electrochemistry 1
flashcards for neet chemistry dec13 electrochemistry 2
flashcards for neet chemistry dec13 electrochemistry 3
flashcards for neet chemistry dec13 electrochemistry 4



Galvanic Cell

Converts the chemical energy released during redox reaction into electrical energy

E.g. Daniell cell

Zn(s) + Cu2+(aq) β†’ Zn2+(aq) + Cu(s)

Cell Electromotive Force (emf)

The potential difference between the two electrodes of a galvanic cell, i.e. of the cathode and anode.

Cathode – reduction (right)

Anode – oxidation (left)

Ecell = Eright – Eleft

Nernst Equation

For the electrode reaction:

Mn+(aq) + ne β†’ M(s)

E(Mn+/M) = EβŠ–(Mn+/M) – RT/nF ln 1/[Mn+]

Equilibrium Constant

from Nernst Equation

EβŠ–cell = 2.303RT/nF log Kc

R is gas constant (8.314 JK-1 mol-1 )

F is Faraday constant (96487 C mol-1)

Kc is equilibrium constant

Gibbs Energy of the Reaction for an Electrochemical


βˆ†rG = – nFE(cell)

E(cell) – emf of the cell

nF – the amount of charge passed

βˆ†rG – Gibbs energy of the reaction

Faraday’s Laws of Electrolysis

First Law: The amount of chemical change produced by the current is proportional to the quantity of electricity passed through the electrolyte

Faraday’s Laws of Electrolysis

Second Law: The amounts of chemical changes produced by the same quantity of electricity in different substances are proportional to their chemical equivalent weights

Primary Batteries

It cannot be reused.

E.g. Dry cell or Leclanche cell

Anode: Zn(s) β†’ Zn2+ + 2e–

Cathode: MnO + NH4+ + e– β†’ MnO(OH) + NH3

Mercury Cell

Primary battery

Anode: zinc – mercury amalgam

Cathode: a paste of HgO and carbon

Secondary Batteries

It can be used again by recharging.

E.g. Lead storage battery

Anode: lead

Cathode: PbO2

Electrolyte: 38% sulphuric acid

Nickel-cadmium Cell

Secondary cell


Reaction during discharge:

Cd(s) + 2Ni(OH)3(s) β†’ CdO(s) + 2Ni(OH)2(s) + H2O(l )

Get access to the full set of flashcards for NEET Chemistry, only at BYJU’S.

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