# Electrochemistry

## Ohm's Law

$$v = IR$$ $$R = \rho \frac{l}{a}$$ $$\text {Where V is Potential difference,}$$ $$\text {R is Resistance,}$$ $$\text {I is current,}$$ $$\text {ρ is specific resistance,}$$ $$\text {l is lenght of conductor and }$$ $$\text {a is the cross-section of conductor.}$$

### Conductance

$$G = \frac{1}{R}$$ $$\text {The specific conductance k =} \frac{1}{\rho}$$ $$\text { Cell constant } \rho = \frac{l}{a}$$ $$k = G. \sigma$$

### Molar conductance

$$\text {Molar conductance }A_{\,M} ( \Phi _{\,C}) = \frac{\text {1000 x k}}{\text{ C (or M)}}$$ $$\text {where C is concentration of electrolyte in terms of molarity.}$$

### Equivelant conductance

$$\text {Equivelant conductance }A_{\,M} (A _{\,C}) = \frac{\text {1000 x k}}{\text{ C (or N)}}$$ $$\text {where C is concentration(normality)}$$ $$A_M = A_{N} \text { x}(n-factor)$$ $$A _{\,o} = \lim_{C \to 0} A _{\,C}$$ $$\text {where} A _{\,o} = \text {equivalent conductance at infinite dilution.}$$

### Faraday's first law of electrolysis

$$m = Zit$$ $$\text {where m is mass of substance deposited, }$$ $$\text {Z is electrochemical equivalent,}$$ $$\text {i is current and}$$ $$\text {t is time.}$$ $$Z = \frac {\text{Atomic mass}}{\text{n x F}}$$ $$\text {Faraday's second law of electrolysis}$$ $$\frac {m _{\,1}} {m _{\,1}} = \frac {E _{\,1}} {E _{\,1}}$$ $$\text {where E is equivalent weight.}$$