Be sure to answer all parts. The air in a hot-air balloon at 785 torr is heated from 15.0°C to 41.0°C. Assuming that the moles of air and the pressure remain constant, what is the density of the air at each temperature? (The average molar mass of air is 29.0 g/mol.)
Density at 15.0°C g/L?
Density at 41.0°C g/L?
1)
P= 785.0 torr
= (785.0/760) atm
= 1.0329 atm
T= 15.0 oC
= (15.0+273) K
= 288 K
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:
1.0328947368421053 atm *29.0 g/mol = density * 0.08206 atm.L/mol.K *288.0 K
density = 1.2674 g/L
Answer: 1.27 g/L
2)
T= 41.0 oC
= (41.0+273) K
= 314 K
USE:
p*molar mass=density*R*T
Put Values:
1.0328947368421053 atm *29.0 g/mol = density * 0.08206 atm.L/mol.K *314.0 K
density = 1.16 g/L
Answer: 1.16 g/L
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