Question

A rubber balloon containing 1.0 L of gas is carried from the top of a mountain to the bottom of the mountain, where it’s volume is measured as .85 L at standard pressure. Assuming that there was no temperature change during the trip, what was the pressure in atmospheres at the top of the mountain?

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Answer 1

the pressure at the top of the mountain was 0.85 atm.

Step-by-step explanation:

We can use the combined gas law to solve this problem:

(P1 * V1) / (T1) = (P2 * V2) / (T2)

where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.

Assuming that the temperature remains constant, we can simplify the combined gas law to:

P1 * V1 = P2 * V2

where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Substituting the given values, we get:

P1 * 1.0 L = 1 atm * 0.85 L

P1 = (1 atm * 0.85 L) / 1.0 L

P1 = 0.85 atm