Assignment:
When phosphorus is burnt in a free supply of air, diphosphorous pentoxide is formed. During later stages of combustion in a limited supply of air, the flame becomes larger greenish and flickering. Another phosphorus oxide is formed which is a white waxy crystalline solid which melts @ 23.8 degrees C and becomes a gas @ 176 degrees C.
a) When the composition of the waxy crystalline solid is determined it is found to contain 56.4% phosphorus by mass, the remainder being oxygen. Use the % composition together with the atomic mass relative to oxygen to obtain the empirical formula of the compound.
At 200 degrees C and a pressure of 760 mmHg, a sample of the oxide with a mass of 0.568g has a volume of 99.5cm3
b) Calculate the volume, in cm3 that the sample would have @ STP, assuming that it remains gaseous.
c) Calculate the density in g/litre, of the gaseous oxide of phorphorus @ STP.
d) Determine the molecular formula of the oxide of phosphorous when it is in the gaseous state.
Provide complete and step by step solution for the question and show calculations and use formulas.