Electrochemistry Class 12 One Shot | CBSE NEET JEE

Electrochemistry Class 12 One Shot | CBSE NEET JEE | chapter 3

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Timestamp:
00:00 Presentation
0:51 Electrochemistry
9:21 Basics of electrochemistry
15:27 Reducing oxidation: memory tip
16:29 Electrochemical cell
4:58 p.m. Daniell cell
32:54 Galvanic or voltaic cell
33:49 Galvanic cell: Redox couples
36:32 Standard electrode potential
41:36 Cellular potential/Cellular electromotive force
43:55 Galvanic cell: Representation
51:56 Half-cell electrode potential
53:34 Standard Hydrogen Electrode (SHE)
57h00 Measure the potential of the Zn:SHE electrode
1:04:41 Measuring the electrode potential of Cu:SHE
1:07:03 Standard electrode potential: Importance
1:07:21 Nernst equation
1:16:36 Nernst equation: Application
1:17:01 Nernst equation: Finding the electromagnetic force of a cell
1:19:24 Nernst equation: Equilibrium constant
1:25:17 Nernst equation: Gibbs free energy
1:29:14 Problem 1.
1:38:08 Problem 2.
1:41:45 Problem 3.
1:47:00 Conductance of electrolyte solution
1:49:48 Conductors, semiconductors and insulators
1:50:31 Metallic conductance
1:53:32 Electrolytic conductance
1:56:29 Electrolytic and metallic conductance
1:57:22 Conductivity of the ionic solution
1:58:53 Conductivity cell
2:01:05 Molar conductivity of the ionic solution
2:04:56 Conductivity: Problem
2:07:59 Variation of conductivity and molar conductivity
2:09:14 Conductivity variation
2:15:23 Molar conductivity variation
2:20:34 Strong electrolytes: molar conductivity
2:27:44 Strong electrolytes: Kohlrausch's law
2:29:28 Low electrolytes
2:34:09 Problem 1
2:36:13 Problem 2

In this video we will cover:
1.NCERT Class 12 Chemistry Electrochemistry Notes
2. NCERT Class 12 Chemistry Electrochemistry Solutions
3.Difference between electrochemical and electrolytic cell?
4. Write the Nernst equation and the electromotive force of the following cells at 298 K:
(a) Sn(s)|Sn2+(0.050 M)||H+(0.020 M)|H2(g) (1 bar), (b) Pt(s) Pt(s),Br2(l)|Br–( 0.010M)||H+(0.030M)| H2(g) (1 bar),Pt(s).
5. Using standard electrode potentials, predict whether the reaction between the following is feasible: Fe3+(aq) and I–(aq)
6. Calculate the standard cell potentials of a galvanic cell in which the following reactions take place:
2Cr(s) + 3Cd2+(aq) → 2Cr3+(aq) + 3Cd. Calculate the ΔrG and the equilibrium constant of the reactions.
7. The electrical resistance of a column of 0.05 mol L–1 NaOH solution with a diameter of 1 cm and a length of 50 cm is 5.55 × 103 ohm. Calculate its resistivity, conductivity and molar conductivity
8. Calculate Ëm° for CaCl2 and MgSO4
9. The conductivity of a 0.20 M KCl solution at 298 K is 0.0248 S cm–1. Calculate its molar conductivity.

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