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A helium balloon with a volume of 2.75 L and pressure of 1.04 atm and 27 °C flies in the sky and reaches an altitude where the temperature is -15 °C and the pressure is 0.530 atm. Calculate the final volume of the balloon

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SouthernRider

Answer:

4.64 L

Explanation:

Given Initial pressure (P1) = 1.04 atm , initial volume (V1) = 2.75L and initial temperature (T1) = 27C = 273+27 = 300K

Also given that final pressure (P2) = 0.530 atm , final temperature (T2) = 15C = 273-15 = 258 K and let the final volume be (V2) = V

We know that an ideal gas follows PV=nRT

Here n and R are constant

so [tex]\frac{PV}{T} = constant[/tex]

[tex]\frac{P1V1}{T1} =\frac{P2V2}{T2}[/tex]

[tex]\frac{1.04\times 2.75}{300} =\frac{0.53\times V}{258}[/tex]

V = 4.64L

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