A completely sealed container holds a mixture of dihydrogen () and dioxygen () at a total pressure o — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

Assume a total mass of $100\text{ g}$. Mass of $H_2 = 20\text{ g}$, Mass of $O_2 = 80\text{ g}$. Moles of $H_2 = 20 / 2 = 10\text{ mol}$. Moles of $O_2 = 80 / 32 = 2.5\text{ mol}$. Total moles = $10 + 2.5 = 12.5\text{ mol}$. Mole fraction of $H_2 = 10 / 12.5 = 0.8$. Partial pressure of $H_2 = \chi_{H_2} \times P_{total} = 0.8 \times 1.0\text{ bar} = 0.8\text{ bar}$. Multiplying by 10 gives $8$.