Question

A weather balloon contains 12.0 m3 of hydrogen gas when it is released from a location at which the temperature is 22°c and the pressure is 101 kpa. it rises to a location where the temperature is -30°c and the pressure is 20 kpa. if the balloon is free to expand so that the pressure of the gas inside is equal to the ambient pressure, what is the new volume of the balloon?

Answer 1

By ideal gas equation we can say

PV = nRT

P = pressure

V = volume

n = number of moles

R = avagadro gas constant

T = temperature

So from above expression we can see that for constant number of moles we can say

`(P_1V_1)/(T_1) = (P_2V_2)/(T_2)`

`(101*12)/(273+22) = (20*V_2)/(273-30)`

`4.11 = 0.082*V_2`

`V_2 = 50 m^3`

So finally the volume will be 50 m^3