Gas Laws and Ideal Gas Equation Notes

## Gas Laws - **Boyle’s Law** (constant T and n): p*1V*1 = p*2V*2 - **Charles’s Law** (constant p and n): \frac{V*1}{T*1} = \frac{V*2}{T*2}- Implication: Absolute minimum temperature exists. - **Avogadro’s Law** (constant T and p): V \propto n ## Absolute Temperature - Kelvin scale: Temp \space in \space °C + 273.15 = Temp \space in \space K ## Ideal Gas Equation - Combination of gas laws: pV = nRT- R (Ideal Gas Constant) = 8.314 \space L \cdot kPa \cdot K^{-1} \cdot mol^{-1} ## General Gas Equation - When the number of moles is constant:
\frac{p*1V*1}{T*1} = \frac{p*2V*2}{T*2} ## Density of Gases - Density (d) = \frac{m}{V} - Density of a gas is proportional to its molecular mass (M). - Using the Ideal Gas Equation:
d = \frac{m}{V} = \frac{pM}{RT} - Dry air: - Average M = 29 \space g \cdot mol^{-1} - Density ≈ 1.2 \space g \cdot L^{-1} - Gases with higher M than 29 (e.g., CO*2, SO*2) sink. - Gases with lower M than 29 (e.g., H*2, He, CO, NH*3) rise.