The pressure exerted on a 240. mL sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?

141.88

P1V1 = P2V2

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

The combined gas law formula is:

(P1 * V1) / T1 = (P2 * V2) / T2

Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature

In this case, the temperature is constant, so T1 = T2. Here are the given values:

P1 = 0.428 atm
V1 = 240 mL
P2 = 0.724 atm

We are looking for V2, the final volume.

Let's substitute the values we have into the combined gas law equation:

(0.428 atm * 240 mL) / T1 = (0.724 atm * V2) / T2

Since the temperature is constant, we can cancel out T1 and T2:

(0.428 atm * 240 mL) = (0.724 atm * V2)

Now, isolate V2:

V2 = (0.428 atm * 240 mL) / (0.724 atm)

V2 = 170.494505 mL

Therefore, the final volume of the sample will be approximately 170.494505 mL.

To find the final volume of the sample, we can use Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional, as long as the temperature remains constant.

Boyle's Law equation is written as follows:

P1 * V1 = P2 * V2

Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume

Let's assign the given values to the variables:

P1 = 0.428 atm
V1 = 240 mL
P2 = 0.724 atm
V2 = ?

Now we can plug in the values into the equation and solve for V2:

P1 * V1 = P2 * V2

0.428 atm * 240 mL = 0.724 atm * V2

103.2 atm·mL = 0.724 atm * V2

To isolate V2, we divide both sides of the equation by 0.724 atm:

V2 = (103.2 atm·mL) / 0.724 atm

V2 ≈ 142.6 mL

Therefore, the final volume of the hydrogen gas sample will be approximately 142.6 mL.