In the determining molar volume experiment, we will use water. how will vapor pressure play a role in this experiment?

The sample's volume is affected by the transferring molecules to the vapor phase, underestimating it.

Explanation:

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Molar properties are said to be measured per unit of mole of the involved substance; more specifically speaking, the molar volume accounts for the volume occupied per mole of the considered substance. In this case, since the affection of the vapor pressure is mean to be explained, we should assume that the experiment is carried out to determine a liquid's molar volume, in such a way, when performing the experiment one must remember that all the liquids have a vapor pressure associated with the pressure exerted by the in-equilibrium molecules of its vapor phase, besides, the vapor pressure causes the liquid to slowly boil as the time go by. In this manner, the vapor pressure could diminish the liquid's molar volume as it is progressively boiled causing an underestimation.

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the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.