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A weather balloon is filled with helium to a volume of 1.61 L at 734 torr. What is the volume of the balloon after it has been released and its pressure has dropped to 0.844 atm? Assume that the temperature remains constant.



Answer :

This answer to this problem can be solved by using Boyle's law.

Boyle's law- This law states that, at constant temperature (in kelvin) the pressure exerted by a gas is inversely proportional to the volume occupied by the gas.

                                       P ∝ 1/V

Solving this above equation we can say that,

                                       P₁V₁= P₂V₂

Given,

V₁ = 1.61 L

P₁ = 734 torr

P₂ = 0.844 atm = (0.844 × 760) =641 torr (∵ 1 atm= 760 torr)

Therefore, V₂= P₁V₁/ P₂

= (734 × 1.61)/ 641= 1.84 L

The volume of the balloon after release of pressure is 1.84 L

Learn more about Boyle's law here-

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