[ktMSU40]

Ok, I have no idea how to do this problem...if someone could just help me start it, I think I can figure it out.

A compound of nitrogen and sulfur was burned in oxygen to produce nitrogen dioxide and sulfur dioxide. The number of moles of nitrogen dioxide produced was 3 times the number of moles of sulfur dioxide produced. What is the empirical formula of the compound? For example, if the empirical formula for the compound contains 2 nitrogen atoms and 3 sulfur atoms, enter N2S3.

Thanks in advance!

[movies]

The empirical formula is just the ratio between equivalents of each atom that is present.  How many N atoms do you have per S?

[Donaldson Tan]

let the compound be N_xS_y where x and y are positive integers

N_xS_y + (x+y)/2 O₂ -> x NO₂ + y SO₂

The number of moles of nitrogen dioxide produced was 3 times the number of moles of sulfur dioxide produced.

y/x = 3
y = 3x

Emperical Formula of the Nitrogen-Sulphur Compound: NS₃