At 89.85 degree Celsius, a 100.0-ml sample of ammonia gas exerts a pressure of 6.90 atm. Assume ideal gas behavior, and calculate the mass of ammonia (NH3) in the sample.
Ideal gas equation is expressed as
PV = nRT
P = pressure = 6.90 atm
V = volume = 100 mL = 0.1 L
R = gas constant = 0.082057 L atm mol-1 K-1
T = 89.85 oC = (89.85 + 273) K = 362.85 K
n = number of moles = ?
Now, substituting the values in the ideal gas equation, we get;
PV = nRT
n = PV / RT
= [ (6.90 atm) (0.1 L) ] / [ (0.082057 L atm mol-1 K-1) (362.85 K) ]
= 0.0232 mol
Now,
Molar mass of NH3 = 17 g/mol
So, 1 mole of NH3 = 17 g
0.0232 mole of NH3 = 0.0232 x 17 g
= 0.3944 g
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