Considering the ideal gas law, at 204.878 K will 4.00 moles of gas occupy a volume of 12.0 L at a pressure of 5.60 atm.
An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.
The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P×V = n×R×T
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances. The numerical value of R will depend on the units in which the other properties are worked.
In this case, you know:
- P= 5.60 atm
- V= 12 L
- n= 4 moles
- R= 0.082 [tex]\frac{atmL}{molK}[/tex]
- T=?
Replacing in the ideal gas law:
5.60 atm×12 L = 4 moles×0.082[tex]\frac{atmL}{molK}[/tex]×T
Solving:
[tex]T=\frac{5.60 atmx12 L}{4 moles x 0.082 \frac{atmL}{molK}}[/tex]
T=204.878 K
Finally, at 204.878 K will 4.00 moles of gas occupy a volume of 12.0 L at a pressure of 5.60 atm.
Learn more about the ideal gas law:
- https://brainly.com/question/4147359?referrer=searchResults
