posted by confused on .
Kc=5.85x10^-3 at 25 degrees C for the reaction
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.
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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.
what does it mean when it says the percentage of the original N2O4 that is dissociated.
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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 = ??