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(B) Boyle's law states that for a fixed mass of an ideal gas at constant temperature, the product of pressure and volume is constant $(PV = 	ext{cons

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Mass of air does not remain constant

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(B) Boyle's law states that for a fixed mass of an ideal gas at constant temperature, the product of pressure and volume is constant $(PV = 	ext{constant})$.When you blow air into a balloon, you are adding more air molecules into the balloon. Therefore, the number of moles $(n)$ of the gas is not constant.According to the ideal gas equation, $PV = nRT$.Since the temperature $(T)$ is constant and the number of moles $(n)$ increases as you blow air into the balloon, the product $PV$ must increase $(PV \propto n)$.Because the mass (and thus the number of moles) of the air inside the balloon does not remain constant, Boyle's law is not applicable.

When air is filled in a balloon, both the pressure and volume increase while the temperature remains constant. Why is Boyle's law not obeyed in this case?

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