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30 May, 00:03

A helium balloon has a volume of 735 mL when it is at ground level. The balloon is

transported to an elevation of 5km, where the pressure is only 0.8atm. At this altitude the gas

occupies a volume of 1286mL. Assuming the temperature has remained the same, what was

the ground level pressure?

O

A.

1.4atm

OB. 0.7atm

O c. 12am

OD. 1.0atm

+3
Answers (1)
  1. 30 May, 03:30
    0
    The answer to your question is P1 = 1.4 atm

    Explanation:

    Data

    Volume 1 = V1 = 735 ml

    Pressure 1 = P1 = ?

    Volume 2 = V2 = 1286 ml

    Pressure 2 = P2 = 0.8 atm

    Process

    To solve this problem use Boyle's law.

    P1V1 = P2V2

    -Solve for P1

    P1 = P2V2 / V1

    -Substitution

    P1 = (0.8 x 1286) / 735

    -Simplification

    P1 = 1028.8 / 735

    -Result

    P1 = 1.4 atm
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