An ideal gas is represented with the equation:
P*V = n*R*T
From this, we will find that the correct option is 2:
"An increase in pressure causes particles to move closer together, decreasing the volume."
Again, the ideal gas equation is:
P*V = n*R*T
where:
P = pressure
V = volume
n = number of moles
R = constant of the ideal gas
T = temperature.
if we divide both sides by n, we get:
P*V/n = R*T
P*v = R*T
Where v is the molar volume.
Now, what does happen if the pressure increases and the temperature is held constant?
To see this, we need to isolate v:
v = (R*T)/P
Remember that T is held constant, and R is a constant. Then we have an inversely proportional relation between v and P.
Thus, if P increases, then v decreases.
If v decreases it means that the molar volume decreases, thus the molecules move close together.
Then the correct option is 2:
"An increase in pressure causes particles to move closer together, decreasing the volume."
If you want to learn more, you can read:
https://brainly.com/question/12414404
