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Which statement explains the molecular changes that occur in an enclosed gas as the pressure increases and the temperature is held constant?

1. An increase in pressure causes particles to move closer together, increasing the volume.

2. An increase in pressure causes particles to move closer together, decreasing the volume.

3. An increase in pressure causes particles to move farther apart, increasing the volume.

4. An increase in pressure causes particles to move farther apart, decreasing the volume.

Sagot :

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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

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