A gas bubble has a volume of $0.650$ mL on the seafloor at a pressure of $3.46$ atm.
What would be its volume at the surface, supposing that seawater would be at the same temperature everywhere?
At the surface we have a pressure of $1$ atm.
Since the temperature remains constant, the ideal gas law falls back to the law of Boyle-Mariotte:
$P_1V_1$ $=$ $P_2V_2$
$V_2$ $=$ $\frac{P_1V_1}{P_2}$ $=$ $\frac{3.46\cdot 0.00065}{1}$ $=$ $2.24\cdot 10^{-3} L$ $=$ $2.24$ mL
