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N2O4(g) = 2NO2(g)
The equilibrium constant Kc at 25C is 0.125. What percentage of dinitrogen tetroxide is dissociated when 0.0330 mol N2O4 is placed in a 1.00-L flask at 25C?
alright so here's what i'm doing
[NO2] = n
[N2O4] = m
n + m = .033
m = .033 - n
.125 = (n^2)/(.033-n)
n = .0271172
[N2O4] = .0058827584
[NO2] = .0271172
now since the volume is 1L the concentrations and the number of moles of each compound is the same. Whether are take the number of moles converted to NO2 and divide it by the original amount or convert the moles of the substances to grams i still get 82% as being converted. This isn't right and i have no idea why. Does anyone know how to solve this question?
The equilibrium constant Kc at 25C is 0.125. What percentage of dinitrogen tetroxide is dissociated when 0.0330 mol N2O4 is placed in a 1.00-L flask at 25C?
alright so here's what i'm doing
[NO2] = n
[N2O4] = m
n + m = .033
m = .033 - n
.125 = (n^2)/(.033-n)
n = .0271172
[N2O4] = .0058827584
[NO2] = .0271172
now since the volume is 1L the concentrations and the number of moles of each compound is the same. Whether are take the number of moles converted to NO2 and divide it by the original amount or convert the moles of the substances to grams i still get 82% as being converted. This isn't right and i have no idea why. Does anyone know how to solve this question?