Gas Laws: Relationships Among Pressure, Volume, and Temperature

A scuba diver releases a 0.75 L air bubble at a depth where the pressure is 2.25 atm. As the bubble rises to the surface, the pressure decreases to 1.03 atm. Assuming temperature remains constant, what is the volume of the bubble at the surface? (Use Boyle’s Law: $P_1V_1 = P_2V_2$)

Which of the following best describes the relationship between pressure and volume for a fixed amount of gas at constant temperature, according to Boyle’s Law?

A helium balloon has a volume of 2.32 L at 40.0°C. If the temperature rises to 75.0°C at constant pressure, what is the new volume? (Use Charles’s Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$, with temperatures in Kelvin)