A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant?
A)580 mL
B)630 mL
C)100 mL
D)110 mL
E)1100 mL

Question

Quizplus · Accepted Answer

We can use the combined gas law formula to solve for the new volume:

(P1V1/T1) = (P2V2/T2)

Where:
P1 = 2.4 atm (initial pressure)
V1 = 250 mL (initial volume)
T1 = 15 °C + 273 = 288 K (initial temperature in Kelvin)
P2 = 1.0 atm (final pressure)
V2 = unknown
T2 = 27 °C + 273 = 300 K (final temperature in Kelvin)

Plugging in the values, we get:

(2.4 atm)(250 mL)/(288 K) = (1.0 atm)(V2)/(300 K)

Solving for V2:

V2 = (2.4 atm)(250 mL)(300 K)/(1.0 atm)(288 K) = 630 mL

Therefore, the volume of the bubble when it reaches the surface is 630 mL. Answer choice B is correct.

A Diver Exhales a Bubble with a Volume of 250