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A 10,0-L cylinder of gas is stored at room temperature (20.0°C) and a pressure of 1800 psi. If the gas is
transferred to a 6.0-L cylinder, at what temperature in CELCIUS would it have to be stored in order for the
pressure to remain at 1800 psí? Reminder, convert your temperature to Kelvin before you begin the problem.
(Please put units)

Sagot :

CintiaSalazaridn

Considering the Charles' law, the gas would have a temperature of -109.2 C.

Charles' law

Finally, Charles' law establishes the relationship between the volume and temperature of a gas sample at constant pressure. This law says that the volume is directly proportional to the temperature of the gas. That is, if the temperature increases, the volume of the gas increases, while if the temperature of the gas decreases, the volume decreases.

Charles' law is expressed mathematically as:

[tex]\frac{V}{T} =k[/tex]

If you want to study two different states, an initial state 1 and a final state 2, the following is true:

[tex]\frac{V1}{T1} =\frac{V2}{T2}[/tex]

Temperature of the gas in this case

In this case, you know:

  • P1= 1800 psi
  • V1= 10 L
  • T1= 20 C= 293 K (being 0 C= 273 K)
  • P2= 1800 psi
  • V2= 6 L
  • T2= ?

You can see that the pressure remains constant, so you can apply Charles's law.

Replacing in the Charles's law:

[tex]\frac{10 L}{293 K} =\frac{6 L}{T2}[/tex]

Solving:

[tex]\frac{10 L}{293 K} T2=6 L[/tex]

[tex]T2=\frac{6 L}{\frac{10 L}{293 K} }[/tex]

T2=163.8 K= -109.2 C

The gas would have a temperature of -109.2 C.

Learn more about Charles's law:

https://brainly.com/question/4147359?referrer=searchResults

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