Considering the ideal gas law, the temperature is 47.58°C.
Definition of Ideal Gas Law
Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.
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. The universal constant of ideal gases R has the same value for all gaseous substances.
- n is the number of moles of the gas.
Temperature in this case
In this case you know:
- P= 0.853 atm
- V= 24.5 L
- n= 0.795 moles
- R= 0.082 atmL/ molK
- T= ?
Replacing in the ideal gas law:
0.853 atm×24.5 L = 0.795 moles×0.082 atmL/ molK×T
Solving:
(0.853 atm×24.5 L)÷ (0.795 moles×0.082 atmL/ molK)= T
320.58 K= 47.58 °C= T (being 273 K= 0°C)
Finally, the temperature is 47.58°C.