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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: ktMSU40 on September 14, 2004, 03:16:11 PM

Title: empirical formula
Post by: ktMSU40 on September 14, 2004, 03:16:11 PM

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! :)

Title: Re:empirical formula
Post by: movies on September 14, 2004, 03:41:24 PM

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

Title: Re:empirical formula
Post by: Donaldson Tan on September 15, 2004, 09:53:13 PM

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

Quote from: ktMSU40 on September 14, 2004, 03:16:11 PM

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