1.

0.2033 g of an organic compound in Dumas method gave 31.7m L of moist nitrogen at 14^(@)C and 758mm pressure. Calculate the percentage of nitrogen in the compound. (Aqueous tension at 14^(@)C=14mm, N= 14)

Answer»

Solution :Pressure due to nitrogen only `=758-14=744mm`
VOLUME of nitrogen at NTP `=(744 xx 31.7 xx 273)/(287 xx 760)`
=29.52mL
Mole of nitrogen `=(29.52)/(22400)`
Weight of nitrogen `(N_(2))= (29.52)/(22400) xx 28= 0.0369g`
% of nitrogen `=(0.0369)/(0.2033) xx 100`= 18.16%


Discussion

No Comment Found

Related InterviewSolutions