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Title: Liquid nitrogen trichloride is heated in a 2.87-L closed reaction vessel until it decomposed completely to gas? Post by: zzz1090 on Mar 11, 2012 Liquid nitrogen trichloride is heated in a 2.87-L closed reaction vessel until it decomposed completely to gaseous elements. The resulting mixture exerts a pressure of 704 mmHg at 90.°C .
(a) What is the partial pressure of each gas in the container? nitrogen____mmHg chlorine_____mmHg (b) What is the mass of the original sample? ____g please explain how to do this Title: Liquid nitrogen trichloride is heated in a 2.87-L closed reaction vessel until it decomposed completely to gas? Post by: fire_crystal on Mar 11, 2012 2NCl3 --> N2 + 3Cl2
from the balanced equation, we see that there is 1mole N2 for every 2moles Cl2 mole fraction N2 = 0.33 mole fraction Cl2 = 0.67 704torr x 0.33 = 232.3torr = N2 471.9torr = Cl2 mass: pv=nrt, solve for n n = pv/(rt) n = 0.926atm x 2.87L / (0.0821L-atm/mole-K x 363K) = 0.089moles gas present 0.089 = total moles mole fraction N2 x total moles = moles N2 = 0.33 x 0.089 = 0.0294moles 0.0294moles x 28g/mole = 0.824g N2 mole fraction Cl2 x total moles = moles Cl2 = 0.67 x 0.089 = 0.06moles 0.06moles x 70.9g/mole = 4.23g Cl2 total mass = 5.05g |