At an altitude for which ambient pressure is #0.700*atm#, and a temperature of #270.15*K#, a balloon contains #3.00*mol# of gas... What is the volume of the balloon....?

1 Answer
anor277
Jun 18, 2017

There is no question here, but your neighbour, the balloonist, has filled a balloon with approx. #100*L# volume.

Explanation:

Of course, he may have heated the contents of the balloon somehow, but we must assume #T=270*K#, so..........

#V=(nRT)/P=(3.00*molxx0.0821*(L*atm)/(K*mol)xx270.15*K)/(0.700*atm)#

#~=100*L.#

We have assumed the temperature, and know that the balloon expanded against a #0.700*atm# pressure. Because the balloon is apparently floating, what is the probable filling gas?

Related questions
See all questions in Ideal Gas Law
Impact of this question
2334 views around the world
You can reuse this answer
Creative Commons License