Question

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

Answer 1

4.64 L

Step-by-step 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
`(PV)/(T) = constant`

`(P1V1)/(T1) =(P2V2)/(T2)`

`(1.04* 2.75)/(300) =(0.53* V)/(258)`

V = 4.64L