According to Charles's Gas Law, when the pressure of a system remains the same going from one state (point 1) to another (point 2), increasing the volume from point 1 to point 2 will result in an increase in the temperature of the gas from point 1 to point 2 as well. In equation form,
V1/T1 = V2/T2
It should be noted that the unit of temperature
to be used is Kelvin. Thus, if the temperature is given in degrees Celsius,
first convert it to Kelvin by adding 273.15.
We then have:
30.0 L/ 473.15 K = x L/ 274.15 K
where, x is the new volume of oxygen
After calculating, we obtain x = 17.38
L O2
If 30.0 L of oxygen are cooled from 200ºC to 1°C at constant pressure, then the new volume of oxygen is 0.15 L.
Charle's law of gases states that at constant pressure, volume of the gas is directly proportional to the temperature of the gas, i.e.
V∝T
According to the question, equation becomes:
V₁/T₁ = V₂/T₂, where
V₁ = initial volume of gas = 30 L
T₁ = initial temperature of gas = 200ºC
V₂ = new volume of gas = ?
T₂ = new temperature of gas = 1ºC
On putting all these values on the above equation, we get
V₂ = (30)(1) / 200 = 0.15L
Hence required volume is 0.15 L.
To know more about Charle's law, visist the below link:
https://brainly.com/question/888898
