A balloon is filled with 73 Lof air at 1.3 atm pressure. What pressure is needed to change the volume to 43 L?

Answer 1

We use old Boyle's Law........and get approx. #P_2=2*atm#.

For a given quantity of gas, pressure is inversely proportional to pressure: #Pprop1/V#. And so #PV=k#, and thus #P_1V_1=P_2V_2#.

We solve for #P_2=(P_1V_1)/(V_2)=(73*Lxx1.3*atm)/(43*L)=??atm.#

Is the increase in pressure reasonable, and if so, why?

By signing up, you agree to our Terms of Service and Privacy Policy

Answer 2

Axel Alvarado

To find the pressure needed to change the volume to 43 L, you can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.

Boyle's Law equation:

P1V1 = P2V2

Where: P1 = initial pressure (1.3 atm) V1 = initial volume (73 L) P2 = final pressure (unknown) V2 = final volume (43 L)

Rearranging the equation to solve for P2:

P2 = (P1 * V1) / V2

Substitute the given values:

P2 = (1.3 atm * 73 L) / 43 L

Calculate:

P2 = (94.9 atm * L) / 43 L P2 ≈ 2.21 atm

Therefore, the pressure needed to change the volume to 43 L is approximately 2.21 atm.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.