The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25^$\circ$C is required for burning 1.00 L of hexane (C₆H₁₄, density = 0.660 g/mL) completely, yielding carbon dioxide and water

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The Answer of The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25^$\circ$C is required for burning 1.00 L of hexane (C₆H₁₄, density = 0.660 g/mL) completely, yielding carbon dioxide and water

The Mole Fraction of Oxygen Molecules in Dry Air Is ∘\circ∘

The Mole Fraction of Oxygen Molecules in Dry Air Is $\circ$