We can use the Boyle's Law equation to solve for the new volume:
P1V1 = P2V2
Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
Plugging in the given values, we get:
(2.0 x 10^6 atm)(1.0 x 10^-5 L) = (0.275 atm)(V2)
Solving for V2, we get:
V2 = (2.0 x 10^6 atm)(1.0 x 10^-5 L) / (0.275 atm)
V2 = 72,727.3 L
Therefore, the new volume of the gas at 0.275 atm pressure would be approximately 72,727.3 L.
The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. If we have a 1.0 x 10-5 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
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1 answer