Karmina inflated a balloon at sea level, where the atmospheric pressure was 101.3 kilopascals. the volume of the balloon was 2.15 liters. she then carried the balloon with her to the top of a mountain, where the atmospheric pressure was 83.1 kilopascals. if the temperature was constant and no air leaked out of the balloon, what was the balloon’s volume at the top of the mountain?

- 2.62 L.

Solution:- If we look at the data then temperature is constant and the volume is changing as the pressure is changed. It's Boyle's law, "At constant temperature, the volume of a gas is inversely proportional to the pressure."

The equation used for this law is:

Let's say the new volume is V, plug in the values in the equation:

101.3kPa(2.15L) = 83.1kPa(V)

V = 2.62 L

So, the new volume of the balloon at 83.1 kPa is 2.62 L.

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it is stable as it is in group 0 which have full outer shells of electrons