Milani

Hi, Thanks for your response. I tried your method but am still having some trouble. Do we calculate the mole of all the gases?

It's a practice question for my chem class. Could you please help? I am not understanding what to do as my teacher doesn't teach properly.

Under certain conditions, the well-known fertilizer ammonium nitrate (NH4NO3) explodes according to the following balanced equation: 2NH4NO3(s) → 2N2(g) + 4H2O(g)+ O2(g) Exactly 577 g of ammonium nitrate is placed in a 33.59 L constant-volume container containing dry air at 489.9 kPa and 29 ºC. The container is heated to 456 ºC and an explosive reaction occurs. It may be assumed that the reaction goes to completion. Luckily, the container remains intact after the explosion. Determine the mole fraction of nitrogen (N2) in the gas phase after the explosion. Round your final answer to two significant figures. Data: Assume that the composition of dry air is 79% N2 and 21% O2 by volume.