a sample of nitrogen gas, N2 occupies 3.0L at a pressure of 3.0 atm. what volume will it occupy when the pressure is changed to 0.50 atm and the temperature remains constant?

Think of Boyle's law from the three gas laws. P1V1=P2V2.you have p1, p2 and v1. then it just simple algebra solve for v2.

I agree with Shawn. Plug and chug.

To solve this problem, we can use the combined gas law equation:

P1 * V1 / T1 = P2 * V2 / T2

Where:
P1 = initial pressure (3.0 atm)
V1 = initial volume (3.0 L)
T1 = initial temperature (constant)
P2 = final pressure (0.50 atm)
V2 = final volume (unknown)
T2 = final temperature (constant)

Since the temperature remains constant, T1 = T2. Therefore, we can simplify the equation to:

P1 * V1 = P2 * V2

Now let's plug in the given values and solve for V2:

(3.0 atm) * (3.0 L) = (0.50 atm) * V2

9.0 L atm = 0.50 atm * V2

V2 = (9.0 L atm) / (0.50 atm)

V2 = 18.0 L

Therefore, the nitrogen gas will occupy a volume of 18.0 L when the pressure is changed to 0.50 atm while keeping the temperature constant.

To find the volume of the nitrogen gas at a different pressure, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, assuming the temperature remains constant.

Boyle's Law formula:

P1 × V1 = P2 × V2

Where:
P1 = initial pressure (3.0 atm)
V1 = initial volume (3.0 L)
P2 = final pressure (0.50 atm)
V2 = final volume (unknown)

Rearranging the formula:

P1 × V1 / P2 = V2

Substituting the given values:

(3.0 atm) × (3.0 L) / (0.50 atm) = V2

Calculating:

(9.0 atm·L) / (0.50 atm) = V2

V2 = 18.0 L

Therefore, when the pressure is changed to 0.50 atm while keeping the temperature constant, the nitrogen gas will occupy a volume of 18.0 L.