Respuesta :
Answer:
Answer in explanation
Explanation:
Gases are expected to behave as ideal gases at particular temperature and pressure know as the S.T.P.
At a temperature of 273k and a pressure of 1atm, it is expected that a mole of a gas will occupy a volume of 22.4L. Now, a particular student measured the pressure of a gas at 425K, it is expected that the pressure is different from the one that is supposed to be observed at STP and thus , the measures quite differently
Real gases do not obey the ideal gas law
The pressure is less than predicted because of the attractive forces between the molecules as well as energy is lost during collision of a real gas
Reason:
The ideal gas equation is given as follows;
- P·V = n·R·T
The real gas equation is presented as follows;
- [tex]\left[P + \dfrac{a \cdot n^2}{V^2} \right]\cdot \left[V - n \cdot b\right] = n \cdot R \cdot T[/tex]
The coefficient +a, is the pressure correction factor, given that the pressure of a real gas is lower than that of an ideal, due to the attractive force that exist between the gas molecules that reduces the number of collisions of the molecules with the container's wall when they attract each other
The collisions that occur in real gas involve energy loss, therefore, the molecules tend to be less activated as predicted by the real gas law
Therefore;
- The pressure of the real CO₂ gas is expected to be much lesser than expected and has to be corrected using the correction factor for the value correspond with the predicted value at the given temperature
Learn more here:
https://brainly.com/question/11544900
