What is the new volume of a balloon originally at 755 torr and 5.00 L is placed in a container in which the pressure is increased to 1.25 atm?

Question

Quizplus · Accepted Answer

Use the combined gas law:

(P1V1)/T1 = (P2V2)/T2

Assume the temperature is constant.

(P1V1)/T = (P2V2)/T

P1V1 = P2V2

Convert the initial pressure to atm:

755 torr = 0.993 atm

Plug in the known values:

(0.993 atm)(5.00 L) = (1.25 atm)(V2)

Solve for V2:

V2 = [(0.993 atm)(5.00 L)]/(1.25 atm)

V2 = 3.97 L

What Is the New Volume of a Balloon Originally at 755