An air bubble has a volume of 1.65 cm3 when it is released by a submarine 105 m below the surface of a lake. What is the volume of the bubble when it reaches the surface? Assume the temperature and the number of air molecules in the bubble remain constant during its ascent.
_____________cm3
To solve this question, we can use Boyle's Law, which states that the product of the pressure and volume of a gas is constant, as long as the temperature and the number of gas molecules remain constant.
In this case, the pressure at the bottom of the lake is greater than at the surface due to the weight of the water above the bubble. As the bubble rises to the surface, the pressure exerted on it decreases, causing the volume of the bubble to increase.
We can use the formula derived from Boyle's Law:
P1 * V1 = P2 * V2
where P1 and V1 represent the initial pressure and volume of the bubble at 105 m below the surface, and P2 and V2 represent the final pressure and volume of the bubble at the surface.
Since the number of air molecules and the temperature remain constant, we can assume P1 equals the atmospheric pressure at the surface, which is approximately 1 atm.
On the other hand, P2 is also equal to the atmospheric pressure at the surface.
Now, we can solve for V2:
P1 * V1 = P2 * V2
1 atm * 1.65 cm3 = 1 atm * V2
V2 = 1.65 cm3
Therefore, the volume of the bubble when it reaches the surface is 1.65 cm3.