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A helium weather balloon is filled to a volume of 219 m3 on the ground, where the pressure is 754 torr and the temperature is 298 K. As the balloon rises, the pressure and temperature decrease, so it is important to know how much the gas will expand to ensure that the balloon can uphold the expansion. What is the volume at an altitude of 10,000 m, where the atmospheric pressure is 210. torr and the temperature is 230 K?

Respuesta :

Answer:

[tex]V_2 = 606.9 m^3[/tex]

Explanation:

By ideal gas equation law we know that

PV = nRT

now we know that when balloon rises to certain level then the number of moles will remains same

so we can say

[tex]n_1 = n_2[/tex]

[tex]\frac{P_1V_1}{RT_1} = \frac{P_2V_2}{RT_2}[/tex]

now plug in all data to find the final volume of the balloon

[tex]\frac{754\times 219}{R(298)} = \frac{210 \times V_2}{R(230)}[/tex]

[tex]V_2 = \frac{230\times 754 \times 219}{210 \times 298}[/tex]

[tex]V_2 = 606.9 m^3[/tex]

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