A balloon originally had a volume of 4.39 L at 44°C and a pressure of 729 torr.To what temperature must the balloon be cooled to reduce its volume to 3.78 L if the pressure is constant?

Question

Quizplus · Accepted Answer

We can use the combined gas law to solve this problem, as we are dealing with a constant pressure:

P1V1/T1 = P2V2/T2

We can rearrange this equation to solve for T2:

T2 = (P2V2*T1)/(P1V1)

Plugging in the given values:

T2 = (729 torr * 3.78 L * 44°C)/(4.39 L * 1 atm)

Note that we need to convert the pressure from torr to atm and the temperature from °C to K, using the conversions 1 atm = 760 torr and K = °C + 273.

T2 = (729/760 * 3.78 * (44 + 273))/(4.39)

T2 ≈ 273 K

Converting back to °C, we get:

T2 ≈ 0.0°C

Therefore, the balloon must be cooled to 0.0°C to reduce its volume to 3.78 L.

A Balloon Originally Had a Volume of 4