1)
P = 1.0atm
T = 273 K
density = 1.34 g/L
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T
Put Values:
1 atm * MM = 1.34g/L * 0.08206 atm.L/mol.K *273.0 K
MM = 30.0 g/mol
This is molar mass NO
Answer: NO
2)
P= 1157.5 torr
= (1157.5/760) atm
= 1.523 atm
T= 65.3 oC
= (65.3+273) K
= 338.3 K
Molar mass of CO2,
MM = 1*MM(C) + 2*MM(O)
= 1*12.01 + 2*16.0
= 44.01 g/mol
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T
Put Values:
1.523 atm *44.01 g/mol = density * 0.08206 atm.L/mol.K *338.3 K
density = 2.4145 g/L
Answer: 2.41
3)
P = 0.866atm
T= 29.8 oC
= (29.8+273) K
= 302.8 K
Molar mass of NO,
MM = 1*MM(N) + 1*MM(O)
= 1*14.01 + 1*16.0
= 30.01 g/mol
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T
Put Values:
0.866 atm *30.01 g/mol = density * 0.08206 atm.L/mol.K *302.8 K
density = 1.0459 g/L
Answer: 1.05
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