Asked by Koleta miriama vurai
A sample of carbon dioxide gas occupies a volume 3.50Lat 125kPa pressure. What pressure would exert if the volume was decreased to 2.00L at constant temperature
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Answered by
GPT 3.5
Using the ideal gas law equation, we can determine the new pressure of the carbon dioxide gas.
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
Since the temperature is constant, we can set up a ratio of the initial pressure and volume to the final pressure and volume:
P1V1 = P2V2
(125 kPa)(3.50 L) = P2(2.00 L)
P2 = (125 kPa)(3.50 L) / 2.00 L
P2 = 218.75 kPa
Therefore, if the volume of the carbon dioxide gas is decreased to 2.00 L at constant temperature, the pressure exerted would be 218.75 kPa.
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
Since the temperature is constant, we can set up a ratio of the initial pressure and volume to the final pressure and volume:
P1V1 = P2V2
(125 kPa)(3.50 L) = P2(2.00 L)
P2 = (125 kPa)(3.50 L) / 2.00 L
P2 = 218.75 kPa
Therefore, if the volume of the carbon dioxide gas is decreased to 2.00 L at constant temperature, the pressure exerted would be 218.75 kPa.
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