Question

An 8.5-liter helium balloon sits inside a larger container. The temperature remains constant, and the pressure in the larger container is reduced to 3 atmospheres. As a result, the balloon's volume increases to 26.5 liters. What was the initial pressure, in atmospheres, exerted on the balloon?

A. 1.0 atmospheres
B. 2.0 atmospheres
C. 3.0 atmospheres
D. 4.0 atmospheres

Answer 1

The initial pressure exerted on the balloon was approximately 9.882 atmospheres.

Step-by-step explanation:

To find the initial pressure exerted on the balloon, we can use the ideal gas law:

P1V1/T1 = P2V2/T2

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

Plugging in the given values, we have:

P1(8.5 L)/10.0°C = 3 atm(26.5 L)/10.0°C

Simplifying, we get:

P1 = (3 atm/8.5 L) x (26.5 L/10.0°C) x (10.0°C/1)

P1 = 9.882 atmospheres

Therefore, the initial pressure exerted on the balloon was approximately 9.882 atmospheres.