A 20.4−g sample of dinitrogen monoxide is confined in a 3.44−L vessel. What is the pressure (in atm) at 121 degrees celcius?
Molar mass of N2O = 2*MM(N) + 1*MM(O)
= 2*14.01 + 1*16.0
= 44.02 g/mol
mass of N2O = 20.4 g
we have below equation to be used:
number of mol of N2O,
n = mass of N2O/molar mass of N2O
=(20.4 g)/(44.02 g/mol)
= 0.4634 mol
we have:
V = 3.44 L
n = 0.4634 mol
T = 121.0 oC
= (121.0+273) K
= 394 K
we have below equation to be used:
P * V = n*R*T
P * 3.44 L = 0.4634 mol* 0.08206 atm.L/mol.K * 394 K
P = 4.3554 atm
Answer: 4.36 atm
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