Question

when the temperature of a trapped sample of gas is increased at constant volume:
the average force of molecular collisions --.
the average frequency of molecular collisions --.
the average kinetic energy of the molecules --.
the pressure of the gas --.
question 3
calculate the ro
molecules at 50^{\circ}c
degrees celsius.

Explanation:

When the temperature of a gas increases at constant volume:

• The average kinetic energy of gas molecules is directly proportional to temperature (\(KE=\frac{3}{2}kT\), where \(k\) is Boltzmann's constant and \(T\) is temperature). So, as \(T\) increases, \(KE\) increases.
• Faster - moving molecules (due to higher kinetic energy) collide with more force (force is related to the change in momentum during collisions, and higher - speed molecules have larger momentum changes) and more frequently (since they are moving faster, they hit the container walls more often in a given time).
• According to the ideal gas law \(PV = nRT\), at constant \(V\) (\(V=\text{constant}\), \(n\) and \(R\) are also constants), \(P\propto T\). So when \(T\) increases, \(P\) increases.

Answer:

the average force of molecular collisions increases, the average frequency of molecular collisions increases, the average kinetic energy of the molecules increases, the pressure of the gas increases.