Chemistry question

Question

A hot air balloon is filled with 1.35 × 10^6L of an ideal gas on a cool morning (11∘ C ) . The air is heated to 107∘C . What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

Answer 1

Given:

Initial volume (V1) = 1.35x10⁶ L

Initial temperature (T1) = 11ºC + 273 = 284K

Final temperature (T2) = 107ºC + 273 = 380K

Asked to find:

Find final volume (V2)

Assuming constant pressure, we are dealing with Charles' Law:

V1/T1 = V2/T2

(1.35x10⁶ L)/284K = V2/380K

V2 = 1.81x10⁶ L