Is it possible to find the volume of condensed water by temperature change without knowing the initial pressure of the flask? I found this problem in a practice sheet. The original source doesn't indicate any authorship or whatsoever.

It states the following:


  A sealed container of $\pu{6.24 L}$ in capacity has humid air at $\pu{30 ^\circ C}$ with a $RH=90\%$. The container temperature is then lower to $\pu{27 ^\circ C}$. Find the volume of condensed water. The vapor pressure of water is $\pu{32 mmHg}$ at $\pu{30 ^\circ C}$ and $\pu{27 mmHg}$ at $\pu{27 ^\circ C}$. You can consider that the volume of condensed water is insignificant.


The problem doesn't specifically mentions any other assumptions but I'm assuming that the gas is behaving ideally and since it is referring to water. I will need the density of water, which is $\pu{1 \frac{g}{mL}}$ and the formula weight of water, which is $\pu{18 g mol-1}$.

The strategy which I thought was that the moles of air will remain the same when the vessel is cooled but the total moles will change before and after, as the moles of water initially will be different when the vessel it is cooled.

Then to find the volume what I need to find is that difference in moles and use the formula weight of water and the density to get volume.

However this is a problem because, how can I characterize the vessel if I'm not given an initial pressure?

I'm aware that:

$$RH=\frac{\textrm{partial pressure}}{\textrm{vapor pressure}}\times 100$$

Therefore I can say that the partial pressure for water is:

$$0.9\times \pu{32 mmHg} = \pu{28.8 mmHg}$$

But what I need is the total pressure in the vessel. Is it possible to find it?

If I could find the total moles, what I could do is find the moles of air by difference as follows:

$$n_{air}=n_{t}-n_{water}$$

These moles will not change.

The moles of water could be found by using the ratio of the partial pressure of water to that of the total is equal to the moles of water divided by the total moles.

$$\frac{n_{water}}{n_{total}}=\frac{p_{water}}{p_{total}}$$

But as it can be seen, I'm stuck. I did not included numerical calculations because if I were to use the equation of the ideal gas:

$$PV=nRT$$

What would I had use as the total pressure? Therefore I'm trapped. Is there any way to find what it is being asked?

Edit:

Following the indications by the answer I did the following:

The number of moles of water vapor at $\pu{30 ^\circ C}$ can be found from using the equation of ideal gas:

$\left(0.9\times 32\,mmHg\right)(6.24\,L)=n_{water}(62.4\frac{mmHg\cdot L}{mol\cdot K})(30+273)K$

$n_{water}=0.009505\,mol$

Then the number of moles of water vapor at $\pu{27 ^\circ C}$:

$\left(27\,mmHg\right)(6.24\,L)=n_{water}(62.4\frac{mmHg\cdot L}{mol\cdot K})(27+273)K$

$n_{water}=0.009\,mol$

Then:

$\Delta n_{water}=0.009505-0.009=0.000505\,mol$

From this quantity the grams of water and volume can be obtained using density of water and the formula weight.

$V=0.000505\,mol\times\frac{18\,g}{1\,mol\,\pu{H_{2}O}}\times\frac{1\,mL}{1g}=0.009090\,mL$

Which would be the volume of the condensed water. Judging from the ammount obtained it makes sense that it is a very tiny volume.
This problem is sloppily worded and, technically, it is not possible to give a definitive answer based on the information provided.  But the missing information is not what you think -- you don't need to know the air pressure in the flask.  What's missing are two key pieces:  The degree of humidity ("humid" doesn't mean "saturated") and the volume of water in the flask.  If the flask contains no water, and air that, while humid, is sufficiently below 100% $RH$ at $\pu{30 ^\circ C}$, there might be no water condensation when cooling to $\pu{27 ^\circ C}$ (i.e. you'd just be increasing the $RH$ from some number &lt;100% to a value that, while larger, is still &lt;100%). Alternately, if the flask is initially half liquid water, then the volume of water that condenses would be about half that if the flask instead initially contained a very small volume of liquid water. Thus here is what I think the author meant to ask:


  A sealed container of $\pu{6.24 L}$ contains an equilibrated mixture of air and liquid water at $\pu{30 ^\circ C}$. The container temperature is then lowered to $\pu{27 ^\circ C}$. Find the volume of water that condenses. Assume the volume of liquid water is insigificant relative to the volume of the container.  The vapor pressure of water is $\pu{32 mmHg}$ at $\pu{30 ^\circ C}$ and $\pu{27 mmHg}$ at $\pu{27 ^\circ C}$.


As to how to approach the question, that's straightforward:  You know the partial pressure of the water vapor at each temperature.  You also know the total volume of the air.  Given this, you can determine the number of moles of water vapor at each temperature (using the ideal gas law).  The difference is the number of moles of water that condenses, from which you can then determine the volume of the water that condenses.