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Textbook Q11.93b

Posted: Mon Nov 28, 2016 7:35 pm
by Sydney Wu 2M
"0.020 mol NO2 was introduced into a 1.00-L flask and the reaction 2 NO2(g) <--> N2O4(g) was allowed to come to equilibrium at 298 K. (a) Using information in Table 11.2, calculate the equilibrium concentrations of the two gases. (b) The volume of the flask is reduced to half its original volume. Calculate the new equilibrium concentrations of the gases."

For part (b), the SSM took the initial molar amount of NO2 and did an ICE box from there. Are we supposed to decrease the volume to 0.5-L after it reached equilibrium in a 1.00-L flask (would use values from part a to convert from concentrations to amount of moles, then ICE box it)? Or are (a) and (b) independent Qs from each other?

Re: Textbook Q11.93b

Posted: Mon Nov 28, 2016 10:29 pm
by MayaKhalil_1L
I believe the SSM goes about the problem as is a and b are independent of each other when solving.

Re: Textbook Q11.93b

Posted: Tue Nov 29, 2016 6:23 am
by Sydney Wu 2M
Alright, thanks!