Taking into account the Charles's law, to 94.36 K or -178.64 °C must a sample of helium gas be cooled from 139ºC to reduce its volume from 3.1 L to 0.71 L at constant pressure.
This law states that the volume is directly proportional to the temperature of the gas: for a given sum of gas at constant pressure, as the temperature increases, the volume of the gas increases, and as the temperature decreases, the volume of the gas decreases.
In summary, Charles' law is a law that says that when the amount of gas and pressure are kept constant, the ratio between volume and temperature will always have the same value:
[tex]\frac{V}{T} =k[/tex]
Studying two different states, an initial state 1 and a final state 2, it is satisfied:
[tex]\frac{V1}{T1} =\frac{V2}{T2}[/tex]
In this case, you know:
Replacing in Charles's law:
[tex]\frac{3.1 L}{412 K} =\frac{0.71 L}{T2}[/tex]
Solving:
[tex]\frac{3.1 L}{412 K} T2=0.71 L[/tex]
[tex]T2 =\frac{0.71 L}{\frac{3.1 L}{412 K}}[/tex]
T2= 94.36 K= -178.64 °C
Finally, to 94.36 K or -178.64 °C must a sample of helium gas be cooled from 139ºC to reduce its volume from 3.1 L to 0.71 L at constant pressure.
Learn more about the Charles's law:
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