# chemistry

Kc=5.85x10^-3 at 25 degrees C for the reaction
N2O4(g)<-->2NO2(g)
fifteen(15.0) grams of N2O4 is confined in a 5.00-L flask at 25 degrees C. Calculate(a) the number of moles of NO2 present at equilibrium and(b) the percentage of the original N2O4 that is dissociated.

1. 0
2. 5
1. uhh if i new chemistry i will help but u should post the same question around 5:00 pm tommorow and name the subject ms.sue shes really helpfull and that's when she usally is on hope some1 helps u if not just post agian 2mmorow..:)

posted by catherine
2. Convert 15.0 g N2O4 to moles and that divided by 5.0 L to obtain molarity.

Set up an ICE chart, substitute into Kc expression and solve.

posted by DrBob222
3. what does it mean when it says the percentage of the original N2O4 that is dissociated.

posted by confused
4. oh drbob222 and srasomething???are really helpful 2 luckly u got a respawn:)

posted by catherine
5. When you finish and know the equilibrium concn of N2O4, then (amt N2O4 present in grams/15.0)*100 = ?? I think you will get the percent answer if you use (moles at equil/original moles)*100 = ??

posted by DrBob222
6. .sljck

posted by Anonymous

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