Shaina B.

asked • 04/07/24

chemistry partial pressures

A(n) 972 mL sample of hydrogen was collected over water at 21.0◦C on a day when the barometric pressure was 757 torr. What volume would the dry hydrogen occupy under standard conditions? The vapor pressure of water at 21.0◦C is 19.0 torr. Answer in units of mL.

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Zahid M. answered • 04/07/24

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P1V1 = P2V2 since temperature is constant.


757*952 = 19*V2


V2 = 37929.7 mL

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J.R. S.

tutor
If it were only that easy. First, the temperature isn't constant, nor is the pressure, as final T is 273 and final P is 1 atm (standard conditions). Further, for the dry gas, one must subtract the 19 torr from the pressure (which it looks like you did). I believe the approach is to use the ideal gas law, solve for moles (initial conditions), use the moles of dry gas, and calculate the new volume under standard conditions (273K and 1 atm).
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04/08/24

Zahid M.

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You are right.
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04/08/24

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