The pressure exerted on a 240.0 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?
the pressure exerted on a240ml sample of hydrogen gas at a constant temperature is increased from 0.428atm.what will the final volume of the sample be?
P1V1 = P2V2
To find the final volume of the sample, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
Boyle's Law can be expressed as: P1 * V1 = P2 * V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume
Let's plug in the given values:
P1 = 0.428 atm
V1 = 240.0 mL
P2 = 0.724 atm
V2 = ?
Using the formula, we can rearrange it to solve for V2:
V2 = (P1 * V1) / P2
Now, substitute the known values:
V2 = (0.428 atm * 240.0 mL) / 0.724 atm
V2 = (102.912 mL⋅atm) / 0.724 atm
V2 ≈ 142.23 mL
Therefore, the final volume of the sample will be approximately 142.23 mL.
To determine the final volume of the sample, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when temperature is held constant.
Boyle's Law equation: P1 * V1 = P2 * V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume
Let's rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Now, let's substitute the given values into the equation:
P1 = 0.428 atm
V1 = 240.0 mL
P2 = 0.724 atm
V2 = (0.428 atm * 240.0 mL) / 0.724 atm
Calculating this expression:
V2 = 142.2 mL
Therefore, the final volume of the sample will be 142.2 mL.