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zzz1090 zzz1090
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Posts: 204
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12 years ago
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
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wrote...
12 years ago
2NCl3 Rightwards Arrow 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
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