According to Boyle's Law, what will happen to a sealed bag of chips when taken to high altitudes (such as in the mountains , or in the unpressurized luggage storage section of a plane) and why? Choose the best answer. The increased air pressure in the mountains will cause the bag to crush as the volume of air inside the bag decreases. The decreased air pressure in the mountains will cause the bag to burst open as the volume of air inside the bag increases until it exceeds the capacity of the bag. The volume of air in the bag will not change as long as the bag is not beyond its expiration date. The decreased air pressure in the mountains will cause the bag to crush as the volume of air inside the bag decreases. The increased air pressure in the mountains will cause the bag to burst open as the volume of air inside the bag increases until it exceeds the capacity of the bag.

The decreased air pressure in the mountains will cause the bag to burst open as the volume of air inside the bag increases until it exceeds the capacity of the bag.

Explanation:

First, when a sealed bag of chips is taken to high altitudes, such as in the mountains, the external air pressure decreases. Using this we can plug in the lowered pressure value into Boyle's Law to see what impact this will have on the volume.

[tex]\begin{document}\textbf{Boyle's Law:}~~~\[P_1 V_1 = P_2 V_2\]\begin{itemize} \item \( P_1 \) : Initial pressure of the gas \item \( V_1 \) : Initial volume of the gas \item \( P_2 \) : Final pressure of the gas \item \( V_2 \) : Final volume of the gas\end{itemize}[/tex]

Since both sides are equal at all times, the decrease in pressure P2 will need to result with an increase in the volume V2. Therefore the volume of air inside the bag will increase as a result to the change in pressure.

Note: P1 and V1 represent the initial pressure and volume which means the product of these values should always be the same.