Question

Solid white phosphorus, P4, ignites spontaneously in air at temperatures above 50 degrees Celsius to produce solid diphosporus pentoxide. For an experiment a scientist needs to produce 275kg of diphosphorus pentoxide. If the reaction proceeds with an 82% yield, what is the volume of oxygen gas (in liters) that is required for the process?

Please write balanced equation and all steps so I can follow along and learn. THANKS

Answer 1

To calculate the volume of oxygen gas, we shall assume the most general atmospheric conditions i.e., 298 K temperature and 1 atm pressure.

Also note that molar mass of oxygen gas = 32.0 g/mol

And molar mass of diphosphorus pentoxide = (2×30.97+5×16.0) g/mol = 141.94 g/mol