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    Perfect (ideal) gases

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    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.

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    Solution Preview

    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
    or n=PV/RT
    R= Gas constant= 8.3145 J.mol ^-1K ^-1
    Therefore
    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 ...

    Solution Summary

    The solution calculates mass, volume, temperature using ideal gas equations

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