Ideal Gas law, Highschool level chemistry

[Spirochete]

A sample of carbon dioxide gas is collected over water at 25 degrees Celsius. Vapor pressure of water (l)=23.8 mmHg. Th carbon dioxide and water occupy a volume of 1.80 L at a pressure of 783.0 mmHg. What mass of Carbon dioxide is present?

 

I'm thinking you just use pv=nrt to solve this, and then convert moles into mass. I guess I'm just not sure what pressure to use to get an exact answer.

 

Do you use the pressure of the CO2 only to calculate the number of moles you have? So 783 mmHg-23.8 mmHg = The pressure of CO2?

 

Then take the number you get from that and plug it into pv=nrt?

 

Or do I just use the pressure of 783 mmHg, making the info given about water just extraneous?

 

Thanks for reading!

[swansont]

The sample will contain a mixture of CO2 and water, with the proportions given by the pressures. The info about the water is not extraneous — you want to use the CO2 pressure and you need the water partial pressure to get it, as you have written. (Or, if you want to look at it differently, you could find the relative volumes that would be taken up by each at the overall pressure — you get the same answer)