Question

In an underground natural gas reserve, a bubble of methane gas, CH4, has a volume of 45.0 mL at 1.60 atm. What volume, in milliliters, will the gas bubble occupy when it reaches the surface where the atmospheric pressure is 99.3kPa, if there is no change in the temperature or amount of gas

Answer 1

The ideal gas law relates to the pressure, volume, and temperature of the gas. The volume of the gas bubble at 99.3 kPa is 73.47 mL.

What is Boyle's law?

The inverse relationship between the pressure and the volume of the gas at constant temperature is given by Boyle's law. The formula for the Boyle's law is given as:

$\rm P_{1}V_{1} = P_{2}V_{2}$

Given,

Initial pressure = 1.60 atm

Initial volume =45.0 mL

Final pressure = 0.98 atm (1 atm = 101.325 kPa)

The final volume is calculated as:

1.60 * 45 = 0.98 * V

V = 73.47 mL

Therefore, the volume of the gas bubble is 73.47 mL.

Learn more about Boyle's law here:

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