Answer:
Increases, increases, stays constant.
Explanation:
Gas molecules move faster as they get hotter. So if the volume as well is increased with the temperature, the average molecular velocity for the gas molecules still increase because it is not a variable that depends on volume. The average force of individual collisions between gas molecules increase as well because of the increase in velocity. But the average number of collisions with the wall per second stay the same because of the increase in volume.
I hope this answer helps.
Question:
Options
A) increases, increases, increases
B) increases, increases, decreases
C) increases, decreases, increases
D) increases, decreases, decreases
E) none of the above
Answer:
The correct option is;
A) increases, increases, increases
Explanation:
Here we have the equations of the kinetic theory of gases as follows
[tex]P = \frac{n\times MW \times v^2_{rms}}{3\times V}[/tex].........(1)
[tex]v_{rms} = \sqrt{\frac{3\times R\times T}{MW} }[/tex].........(2)
Where
P = Pressure
[tex]v_{rms}[/tex] = Root mean square velocity
MW = Molecular weight
V = Volume
R = Universal gas constant
T = Temperature
From the above it is seen that when the temperature of the gas is increased the average velocity increases
Also at constant pressure, according to Charles law an increase in temperature will lead to an increase in volume volume
While according to Avogadro's law at constant pressure and temperature, the force of molecule to wall collision is constant increasing the temperature increases the average force and frequency of individual collisions, more so according to equation (2).
