Please help, just help me please 35. Elemental phosphorus burns in oxygen with an intense flame, producing a brilliant light and clouds of the oxide product. These properties of the combustion of phosphor led to its being used in bombs and incendiary de warfare. P4(s) + 502(8) --> 2P205(s) If 4.95 g of phosphorus is burned, what mass of sy it combine with?

I'm gonna assume you want to find how much mass of oxygen 4.95g of phosphorus reacts with

P4(s) + 502(8) --> 2P205(s)

We know that Phosphorus is polyatomic and Oxygen Gas is diatomic

Atomic mass of Phosphorus= 30.97g/mol

Atomic mass for Oxygen = 16g

4 * 30.97 = 123.88g

2 * 16 = 32g

Since there are 5 moles of oxygen: 5 * 32 = 160g

Ok, so 160g of oxygen will react 123.88g of Phosphorus

4.95g phosphorus burns with how much oxygen?

4.95 * 160g

 123.88g

= 6.4g of Oxygen

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :