Question

The highest pressure ever produced in a laboratory setting was about 2.0 x 10° atm. If we have a 1.0 x

10 liter sample of a gas at that pressure, then release the pressure until it is equal to 0.275 atm, what would
the new volume of that gas be?

Answer 1

Step-by-step explanation:

We can use the combined gas law to solve this problem, which relates the initial and final pressure, volume, and temperature of a gas:

P1V1/T1 = P2V2/T2

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

We are given that the initial pressure P1 is 2.0 x 10^30 atm, the initial volume V1 is 1.0 x 10 liters, and we can assume that the temperature remains constant. We are also given that the final pressure P2 is 0.275 atm.

Substituting these values into the combined gas law and solving for V2, we get:

V2 = V1 x (P1/P2) = (1.0 x 10 L) x (2.0 x 10^30 atm / 0.275 atm) = 7.27 x 10^30 L

Therefore, the new volume of the gas at a pressure of 0.275 atm is approximately 7.27 x 10^30 liters.