Question

..A 1.00 L balloon is filled with helium at 1.20 atm. If the balloon is squeezed into a 0.500 L

beaker and doesn't burst, what is the pressure of the helium?
Write out the answer

Answer 1

P₂ = 2.4 atm

Step-by-step explanation:

Given data:

Initial volume = 1.00 L

Initial pressure = 1.20 atm

Final volume = 0.500 L

Final pressure = ?

Solution:

The given problem will be solved through the Boyle's law,

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume

Now we will put the values in formula,

P₁V₁ = P₂V₂

1.20 atm × 1.00 L = P₂ × 0.500 L

P₂ = 1.20 atm. L /0.500 L

P₂ = 2.4 atm