Answer :
The temperature of an 11.2 L sample of carbon monoxide, CO, at 744 torr is 276.21° K or 3.06° C
For given question,
A sample of carbon monoxide (CO) occupies 13.3 l at 55 °c and 744 torr
We know that Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas.
This law says that when the amount of gas and pressure are constant, the quotient between the volume and the temperature will always have the same value:
V/T = k
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 can apply Charles's law because it can be seen that the pressure is constant, with a value of 744 torr at the beginning and end of the analysis. Then, you know:
V₁ = 11.2 L
T₁ = ?
V₂ = 13.3 L
T₂ = 55° C
= 328° K
Replacing in Charles's law:
[tex]\frac{11.2}{T1} =\frac{13.3}{328}[/tex]
We solve above proportion to find the value of T1
⇒ 11.2 × 328 = T1 × 13.3
⇒ 3673.6 = T1 × 13.3
⇒ T1 = 276.21° K
⇒ T1 = 3.06° C
Therefore, the temperature of an 11.2 L sample of carbon monoxide, CO, at 744 torr is 276.21° K or 3.06° C
Learn more about the Charles's law here:
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