A student collects 250 mL of hydrogen gas (H2) over water at 25°C and 1.0 atm. Calculate the volume of dry hydrogen gas (at 25°C and 1.0 atm) that was collected, given the vapor pressure of water at 25°C is 23.8 mmHg.
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To find the volume of dry hydrogen gas, we need to subtract the volume of water vapor from the total volume.
First, let's convert the vapor pressure of water from mmHg to atm:
23.8 mmHg = 23.8/760 atm = 0.0313 atm
Next, we can use Dalton's law of partial pressures to find the partial pressure of hydrogen gas:
Total pressure = pressure of hydrogen gas + pressure of water vapor
1.0 atm = pressure of hydrogen gas + 0.0313 atm
Now, we can solve for the pressure of hydrogen gas:
pressure of hydrogen gas = 1.0 atm - 0.0313 atm = 0.9687 atm
Finally, we can use Boyle's law to find the volume of dry hydrogen gas:
V1/P1 = V2/P2
(250 mL)/(1.0 atm) = V2/(0.9687 atm)
V2 = (250 mL)(0.9687 atm)/(1.0 atm)
V2 ≈ 242.18 mL
Therefore, the volume of dry hydrogen gas collected is approximately 242.18 mL.
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