Solve Gas Law: Volume at STP from Pressure & Temp of Hydrogen Gas

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To determine the volume of hydrogen gas at standard temperature and pressure (STP), the initial conditions of 25°C and 745 mm Hg must be adjusted for the vapor pressure of water, which is 23.8 mm Hg. This means the effective pressure of the dry hydrogen gas is 745 mm Hg - 23.8 mm Hg, resulting in a pressure of 721.2 mm Hg. Using the ideal gas law (PV=nRT), the volume can then be calculated by converting the conditions to STP, where pressure is 760 mm Hg and temperature is 273 K. The initial volume of 43.5 mL cannot be used directly, as it does not represent the gas under STP conditions. The calculations will yield the correct volume of hydrogen gas at STP once the adjustments for pressure and temperature are made.
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Homework Statement


Hydrogen gas is collected over water at 25°C. The atmospheric pressure in the room is 745 mm Hg and the volume of gas in the container is 43.5mL. The vapor pressure of water at 25°C is 23.8 mm Hg. Determine the volume the gas would occupy at STP.


Homework Equations


PV=nRT
PV/NT=PV/NT
standard pressure=760 mm Hg or 1 atm
standard temperature= 273 Kelvin


The Attempt at a Solution


Well for this one I wasn't really sure if they just gave me excess information to throw me off. My first response was to say that the volume would just be 43.5mL. None of the equations provided above worked with just the information given. Is this really as easy at it seems?
 
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No, it is not that easy, and there is no excess information.

First of all, you know the volume at 745 mmHg and 25°C, these are not STP conditions, so the answer can't be 43.5mL.

Then, some of the volume is taken by the water vapor, and you are asked about the volume of just hydrogen - so you have to take 23.8 mmHg into account. What is the pressure of the dry hydrogen in the collected sample?
 

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