Please help im so miffed by this question!
A 1g sample of Hexane was burned completely in Oxygen using EXACTLY double the volume of Oxygen required bt the stoichemetric equation. The resulting gas mixture was collected in a container over water. Calculate the volume of this gas mixture at 20 degrees celsius and 100.5kPa pressure, includind a correction for the vapour pressure of water which is 2.3kPa at 20 degrees celsius.
2006-11-23 10:36:15 · 3 answers · asked by Stevie B 2 in Science & Mathematics ➔ Chemistry
Write the balanced equation - you need the mole ratios.
Change 1g hexane to moles of hexane.
See how many moles of oxygen are USED and how many moles of CO2 and H2O are formed.
Your total number of moles in the reaction mixture would then be:
moles of Oxygen NOT used + moles of CO2 (we will assume the water formed consenses to a liquid at 20 degrees).
Use the Ideal Gas Law to figure out the volume.
PV = nRT
where P = given pressure - water vapor pressure
where V = your unknown
where n = your total moles of gas
where R = the appropriate Universal Gas Law constant
where T = the temperature in KELVIN
2006-11-24 08:00:00 · answer #1 · answered by The Old Professor 5 · 0⤊ 0⤋
I teach chemistry and I could do this problem. But after eating a turkey dinner, it'd be like so much......work. Good luck to you.
2006-11-23 18:56:00 · answer #2 · answered by Anonymous · 0⤊ 1⤋
do your own homework
2006-11-23 18:53:10 · answer #3 · answered by Anonymous · 0⤊ 0⤋