Question

A scuba diver is 45 m below the surface of a lake, where the temperature is 5°C. He releases an air bubble with a volume of 10 cm³. The bubble rises to the surface, where the temperature is 25°C. Assume that the air in the bubble is always in thermal equilibrium with the surrounding water, and assume that there is no exchange of molecules between the bubble and the surrounding water. What is the volume of the bubble right before it breaks the surface? Hint: Remember that the pressure also changes.
A scuba diver is 45 m below the surface of a lake, where the temperature is 5°C. He releases an air bubble with a volume of 10 cm. The bubble rises to the surface, where the temperature is 25°C. Assume that the air in the bubble is always in thermal equilibrium with the surrounding water, and assume that there is no exchange of molecules between the bubble and the surrounding water. What is the volume of the bubble right before it breaks the surface? Hint: Remember that the pressure also changes. x cm Apply the ideal-gas law for a fixed amount of gas. eBook

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Answer 1

h=45m Pi= Patm + Pgh) 5 = 1.01325 X 10° Pa + 1089.884 5 3 5 5.42325X10° Pa Pa = 1.01325x103 Pa V = loum 3 Ti = 5°C= 278K Ta=25°0=298K Using ideal gas law Povi = Pala To Ta =) Vas Pilota Tipa 5,42325 x20 5x 105x10x298 278 X 1.01325 X10 - 57.37 am 3