200 mL of $N_2$ at $25^o C$ and 250 mm of Hg are mixed with 350 mL of $O_2$ at $25^o C$ and 300 mm of Hg in a vessel of capacity 300 mL. Calculate the final pressure of mixture at $25^o C$.

Using Boyle's law, we find the individual pressures of the gases in the 300 mL vessel by calculating P1V1 / V_final for each gas. For nitrogen, the pressure is (250 multiplied by 200) / 300 = 166.67 mm Hg, and for oxygen it is (300 multiplied by 350) / 300 = 350 mm Hg. By Dalton's law of partial pressures, the final pressure is the sum of these partial pressures, 166.67 + 350 = 516.67 mm of Hg.

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