Question

Write the steps please...

A balloon used for atmospheric research has a volume of 3.8×10⁷ L. Assume that the balloon is filled with helium gas at STP and then allowed to ascend to an altitude of 10 km, where the pressure of the atmosphere is 246 mm Hg and the temperature is -36.0 °C. What will the volume of the balloon be under these atmospheric conditions?

Volume= ..............L

Answer 1

Initial Volume of balloon(V1) = 3.8 x 10^7 L

Initial pressure(P1) = 760mm Hg = 1atm

Initial Temperature(T1)= 273K

Final pressure(P2) = 246mm Hg = 0.98atm

Final temperature(T2)= -36°C = 237K

Final Volume(V2) = ?

Using the General gas equation, since we are dealing with gas

(P1xV1)/T1=(P2xV2)/T2

V2= (P1xV1xT2)/(P2xT1)

= (1x3.8x10^7x237)/(0.98x273)

= 3.4x10^7L

Therefore, the volume of the balloon under the stated atmospheric conditions is 3.4x10^7L