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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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smhry smhry
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12 years ago
Liquid nitrogen trichloride is heated in a 2.36 L closed reaction vessel until it decomposed completely to gaseous elements.  the resulting mixture exerts a pressure of 708 mmHg at 87C.  what is the partial pressure of each gas in the container?

nitrogen    mmHg
chlorine    mmHg
what is the mass of the original sample?
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#1
12 years ago
2 NCl3 = N2 + 3 Cl2

partial pressure Cl2 = 3 x partial pressure N2

partial pressure N2 + 3 x partial pressure N2 = 708

x + 3x = 708
x = 177 mm Hg = partial pressure N2
partial pressure Cl2 = 3x = 531 mm Hg
p = 708 /760=0.932 atm
T = 87 + 273 =360 K
Moles N2 + Cl2 = pV / RT = 0.932 x 2.36 / 0.08206 x 360 = 0.0745

moles N2 / 0.0745 = 177 / 708
moles N2 = 0.0186

moles NCl3 = 2 x 0.0186 = 0.0372
mass NCl3 = 0.0372 x 120.366 g/mol= 4.48 g
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