Once you've identified the initial and final conditions, you're ready to solve for the unknown quantity in your problem. Boyle's Law expresses the pressure-volume relationship as P Vi = BV2, so you will need to solve this equation for the unknown quantity and then plug in your known values to calculate the unknown. What pressure would it take to compress 300. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature

Question

Once you've identified the initial and final conditions, you're ready to solve for the unknown quantity in your problem. Boyle's Law expresses the pressure-volume relationship as P Vi = BV2, so you will need to solve this equation for the unknown quantity and then plug in your known values to calculate the unknown. What pressure would it take to compress 300. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature

Answer 1

First you made a typo. You should have written P1V1 = P2V2

Second, I don't understand your problem. All you need to do is to substitute the values in the problem and solve the equation. Here goes.
P1V1 = P2V2
P1 = 1 atm
V1 = 300 L He gas
P2 = unknown pressure in atm. Solve for this.
V2 = 2 L
Plug those values in and solve for P2
P2 = ?
Post your work if you get stuck.

Answer 2

To solve for the unknown pressure, we can rearrange Boyle's Law equation as:

P1 * V1 = P2 * V2

Where:
P1 = initial pressure (1.00 atm)
V1 = initial volume (300. L)
P2 = final pressure (unknown)
V2 = final volume (2.00 L)

Now, let's plug in the given values:

1.00 atm * 300. L = P2 * 2.00 L

To solve for P2, we need to isolate it on one side of the equation. Divide both sides by 2.00 L:

(1.00 atm * 300. L) / 2.00 L = P2

Now, let's calculate the pressure:

P2 = (1.00 atm * 300. L) / 2.00 L

P2 = 150.00 atm

Therefore, it would take a pressure of 150.00 atm to compress 300. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature.

Answer 3

To solve this problem using Boyle's Law, we can use the equation P1V1 = P2V2.

Step 1: Identify the initial and final conditions:
- Initial conditions:
- Volume (V1) = 300. L
- Pressure (P1) = 1.00 atm

- Final conditions:
- Volume (V2) = 2.00 L

Step 2: Solve for the unknown quantity (pressure) and rearrange the equation:
- Rearrange Boyle's Law equation: P1V1 = P2V2

- Plug in the known values: 1.00 atm * 300. L = P2 * 2.00 L

Step 3: Calculate the unknown pressure:
- Solve for P2: P2 = (1.00 atm * 300. L) / 2.00 L = 150. atm

So, the pressure required to compress 300. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature is 150. atm.