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#### ktMSU40

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##### empirical formula
« 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.

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##### Re:empirical formula
« Reply #1 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?

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##### Re:empirical formula
« Reply #2 on: September 15, 2004, 09:53:13 PM »
let the compound be NxSy where x and y are positive integers

NxSy + (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
« Last Edit: September 15, 2004, 09:54:54 PM by geodome »
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