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
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.
To find the new volume of the gas after the pressure is reduced, we can use the combined gas law equation:
P1V1 = P2V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume
Given:
P1 = 2.0 x 10^6 atm
V1 = 1.0 x 10^-5 L
P2 = 0.275 atm
Substituting the values into the equation, we can solve for V2:
(2.0 x 10^6 atm)(1.0 x 10^-5 L) = (0.275 atm)(V2)
(2.0 x 10^6)(1.0 x 10^-5) = 0.275V2
V2 = (2.0 x 10^6)(1.0 x 10^-5) / 0.275
V2 = 7.27 x 10^-3 L
Therefore, the new volume of the gas would be approximately 7.27 x 10^-3 liters.
To find the new volume of the gas, we can use the combined gas law, which states that the initial pressure times the initial volume divided by the initial temperature is equal to the final pressure times the final volume divided by the final temperature. Since we are not given any information about the temperature, we can assume it remains constant.
We are given the following information:
Initial pressure (P1) = 2.0 x 10^6 atm
Initial volume (V1) = 1.0 x 10^-5 L
Final pressure (P2) = 0.275 atm
We need to find the final volume (V2).
Using the combined gas law, we can set up the equation as:
(P1 * V1) / T = (P2 * V2) / T
Since the temperature is constant, we can cancel it out, leaving us with:
P1 * V1 = P2 * V2
Let's substitute the given values into the equation:
(2.0 x 10^6 atm) * (1.0 x 10^-5 L) = (0.275 atm) * V2
Simplifying the equation:
(2.0 x 10^6)(1.0 x 10^-5) = 0.275 * V2
V2 = (2.0 x 10^6)(1.0 x 10^-5) / 0.275
Calculating the value:
V2 = 72727.27 L (rounded to five decimal places)
Therefore, the new volume of the gas after releasing the pressure to 0.275 atm would be approximately 72727.27 liters.