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The ideal gas law is \(PV = nRT\) for n mole of ideal gas.

Here, you have to use Bayle鈥檚 law for this problem.

The initial pressure inside the bag is \({P_1} = 1.00\;{\rm{atm}}\).

The final pressure inside the bag on the airplane is \({P_2} = 0.75\;{\rm{atm}}\).

Let \({V_1}\) and \({V_2}\)bethe initial and final volume of the bag, respectively.

You can assume the temperature does not change.

Now, according to Boyle鈥檚 law, you get the following:

\(\begin{array}{c}{P_1}{V_1} = {P_2}{V_2}\\\frac{{{V_1}}}{{{V_2}}} = \frac{{{P_2}}}{{{P_1}}}\\\left( {\frac{{{V_2} - {V_1}}}{{{V_1}}}} \right) \times 100\% = \left( {\frac{{{P_1} - {P_2}}}{{{P_2}}}} \right) \times 100\% \end{array}\)

Now, substituting the values into the above equation, you getthe following:

\(\begin{array}{c}\left( {\frac{{{V_2} - {V_1}}}{{{V_1}}}} \right) \times 100\% = \left( {\frac{{{P_1} - {P_2}}}{{{P_2}}}} \right) \times 100\% \\ = \left( {\frac{{1.00\;{\rm{atm}} - 0.75\;{\rm{atm}}}}{{0.75\;{\rm{atm}}}}} \right) \times 100\% \\ = 33\% \end{array}\)

Hence, the bag had puffed up\(33\% \) in comparison to when it was packaged.