A mass of 1.663 g of an unknown gas is introduced into an evacuated 2.00 L flask. If the pressure in the flask is 0.544 atm at 78 °C, which of the following gases might be in the flask? (R = 0.08206 L·atm/mol·K)
a. N2
b. N2O
c. C2H2
d. HCl
e. NH3
Answer:
T = 78 + 273 = 351 K
n = pV / RT = 0.544 x 2 / 0.08206 x 351 = 0.0378
moles = mass / molecular mass
molecular mass = mass / moles = 1.663 / 0.0378 = 44 g/mol
It is N2O ( 14 + 14 + 16 = 44 )
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