By going through these Maharashtra State Board 12th Science Chemistry Notes Chapter 5 Electrochemistry students can recall all the concepts quickly.
Maharashtra State Board 12th Chemistry Notes Chapter 5 Electrochemistry
→ Electrical conductance (G) = \(\frac{1}{R}\)Ω-1 2 or S
→ Cell constant = \(\frac{l}{a}\) cm-1 (m-1)
→ Conductivity(k) = \(\frac{\text { Cell constant }}{\text { Resistance }}\)
→ Molar Conductivity(∧m) = \(\frac{\kappa}{C}\) (k in Ω-1 m-1 and C in mol-3) OR
∧m = \(\frac{\kappa \times 1000}{C}\) (k in Ω-1 cm-1 and C in mol dm-3)
→ Kohlrausch’s law : ∧0 = \(\lambda_{+}^{0}+\lambda_{-}^{0}\)
→ Degree of dissociation (α) = \(\frac{\Lambda_{\mathrm{m}}}{\Lambda_{0}}\)
→ Dissociation constant (Ka) = \(\frac{\bigwedge_{\mathrm{m}}^{2} C}{\Lambda_{0}\left(\Lambda_{0}-\Lambda_{\mathrm{m}}\right)}\)
→ 1 Faraday = 96500 C (Change on one mole of electrons)
→ E°cell = E°red (cathode) – E°red (anode)
→ EMn+/M = E°Mn+/M – \(\frac{0.0592}{n}\) log10[Mn+]
→ Ecell = E°cell – \(\frac{0.0592}{n} \log _{10} \frac{[\text { Products }]}{[\text { Reactants }]}\)
→ ΔG° = – nFE°cell
→ ΔG = -nFEcell
→ ΔG°= -RTlnK
→ E°cell = \(\frac{0.0592}{n}\) log10K
For spontaneous cell reaction : Ecell > 0; ΔG < 0