# Amagat law

Amagat law: For a mixture of non-reacting gases the sum of partial volumes of these gases is equal to total volume of the mixture at constant temperature and pressure. $V_{mix} = V_1 + V_2 + V_3 + V_4 \cdots$

Example5. Calculate the volume occupied by 1.0 g of argon at 300 K and $50Nm^{-2}$ pressure. $(\text{mole mass of Ar} 40, R = 8.314 JK^{-1} mol^{-1}$).

Solution: no. of moles of argon, $n = \dfrac{m}{M}$

(m = mass of substance, M = Mol. Wt. of substance) $n = \dfrac{1.0 g}{40 g} \text{mol}^{-1} = 0.025 mol$

According to ideal gas equation, PV = Nrt

Or, $V = \dfrac{Nrt}{p} \\[3mm] = \dfrac{(0.025 mol)(8.314 JK mol^{-1})(300 K)}{50 Nm^{-2}} \\ 1.247 m^3$

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