How do we sketch pressure against pV/T where p is pressure, V is volume and T is temperature?
Answers
Answer:
Gases are composed of minute discrete particles (usually molecules).
Explanation:
Gases are composed of minute discrete particles (usually molecules).
The particles are in continuous chaotic motion moving in straight lines between very frequent collisions with each other and the sides of the container (approximately 109/s).
The bombardment of the container walls by the particles causes the phenomenon we call pressure (i.e. force of impacts/unit area). The greater the force of collision and the more frequent the collisions the greater the gas pressure exerted on the container surface.
The collisions are perfectly elastic i.e. no energy loss on collision due to friction.
At relatively low pressures the average distance between particles is large compared to the diameter of the particles and therefore the inter–molecular forces between the particles is negligible.
The average kinetic energy of the particles is directly proportional to their absolute temperature on the Kelvin scale (K) i.e. KE(J) T(K)
This means if you heat up a gas the average kinetic energy of the particles increases, therefore the average speed increases too.
The Kelvin scale of temperature is explained below.
When a gas behaves according to this model, the gas laws described in sections 4a to 4e are obeyed.
However in real gases things are not so simple and this non–ideal behaviour is discussed in section 5.
Pv vs P graph can be plotted.
