Question

According to the Kinetic Molecular Theory, as the volume of an enclosed gas increases:

the number of particle impacts per unit area increases
the temperature must change
the total number of particle impacts increase
the number of particle impacts per unit area decreases

Answer 1

\[pV = nRT\]

let's keep pressure constant, and number of moles constant.

nR = constant

\[V_{1} = T_{1} nR \]

\[\frac{ V_{1} }{ T_{1} } = nR = \frac{ V_{2} }{ T_{2} }\]

\[\frac{ V_{1} }{ T_{1} } = \frac{ V_{2} }{ T_{2} }\]

If we plot volume and temperature we get a straight line.



if the volume goes up the temperature goes up too.

Answer 2

To test the last claim we need to keep the temperature constant to study pressure and volume.

\[pV = nRT \]

\[P_{1}V_{1} = nR = k = P_{2}V_{2}\]

IF increase the volume or make V_2 bigger, for the two to equal echoer, the pressure must go down. pressure translates to how many times the particles hit the walls of the container
fewer times. so that's also true.

Answer 3

thank you sir
much obliged

Answer 4

Select the TWO variables that are held constant when testing Boyle's Law in a manometer.

pressure
temperature
volume of gas
mass of gas
atmospheric pressure?

Answer 5

i cant decide which one to pick

Answer 6

@23188 no problem, I provided you an explanation for your other question too.