Suppose your balloon has a radius of 3 m and that it is a spere when inflated.
a.) how much H is needed to inflate it to a pressure of 1 atm at an ambient T of 25 celsius @ sea level?
b.) what mass can the balloon lift @sea level, where the density of air is 1.22 kg m^-3 ?
c.) what would be the payload if helium were used instead of hydrogen?
d.) would you and a companion on board, the balloon ascends to 30,000 feet where pressure is 0.28 atm. Assume no volume change, what is the temp (in celsius) at 30,000 feet?
PLEASE- detailed steps, I need to know not just the answer, but understand how you got there- much thanks.© BrainMass Inc. brainmass.com October 24, 2018, 6:25 pm ad1c9bdddf
a.)how much H is needed to inflate it to a pressure of 1 atm at an ambient T of 25 celsius @ sea level?
radius of balloon= 3 m
Volume of balloon= (4/ 3 ) pi r ^3 = 113.10 m^3
Volume=V= 113.10 m^3
Pressure=P= 1 atm= 101350 N / m^2
Temperature= T= 25 C= 298.15 K =273.15+25
Ideal gas Law is PV=nRT
R= Gas constant= 8.3145 J.mol ^-1K ^-1
No of moles=n= 4623.97 moles =(101350*113.1)/(8.3145*298.15)
No of moles required to inflate the balloon= 4623.97 moles
1 mole of Hydrogen ...
The solution calculates mass, volume, temperature using ideal gas equations
Aerodynamics - Perfect Gas Law
Q: If 1500lb of air is pumped into a previously empty 900ft^3 storage tank and the air temperature in the tank is uniformly 70 F, what is the air pressure in the tank in atmospheres?
Is it possible to solve this with the perfect gas law (PV = nRT)? Also, please brief description of the difference between the Ideal Gas Law and the Perfect Gas Law.View Full Posting Details