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)

→ E_{Mn+/M} = E°_{Mn+/M} – \(\frac{0.0592}{n}\) log_{10}[M^{n+}]

→ E_{cell} = E°_{cell} – \(\frac{0.0592}{n} \log _{10} \frac{[\text { Products }]}{[\text { Reactants }]}\)

→ ΔG° = – nFE°_{cell}

→ ΔG = -nFE_{cell}

→ ΔG°= -RTlnK

→ E°_{cell} = \(\frac{0.0592}{n}\) log_{10}K

For spontaneous cell reaction : E_{cell} > 0; ΔG < 0