A 1.58g gaseous sample of C2H3X3 with a volume of 355 mL and 769 mm of mercury at 95 degrees C. What's x?



Answer:
V = 0.355 L
p = 769 / 760 = 1.01 atm
T = 95 + 273 = 368 K
pV = nRT
n = pV / RT = 1.01 x 0.355 / 0.0821 x 368 = 0.0119 moles
1.58 g / 0.0119 = 132.8 g/mol is the molecular weight of the compound
12 + 12 + 1+1+1 = 27
132.8 - 27 = 105.8
105.8 / 3 = 35.3 g/mol ( atomic weight of X )

X is Cl

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