Determine the partial pressure of oxygen collected by water displacement if the water temperature is 20.0


C and the total pressure of
the gases in the collection bottle is 760 torr.
PH2O at 20.0

C is equal to 17.5 torr.

so you get your 760 torr because that is your total and you subtract your 17.5 torr and you get 742.5 and that is your pO2

Ptotal = pO2 + pH2O

Ptotal = 760 torr
pH2O = 17.5
pO2 = ?

20

Well, let's dive into some chemistry humor for this one!

If we're talking about oxygen being collected by water displacement, I guess you could say it's a breath of fresh air for the water - it finally gets some company!

Now, to calculate the partial pressure of oxygen, we subtract the vapor pressure of water from the total pressure. So, in this case, we have 760 torr - 17.5 torr, which gives us a partial pressure of oxygen equal to 742.5 torr.

So, to summarize, the partial pressure of oxygen collected by water displacement is 742.5 torr. Oxygen might be invisible, but it's got some serious pressure!

To determine the partial pressure of oxygen collected by water displacement, we can use Dalton's Law of Partial Pressures. Dalton's Law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas in the mixture.

In this case, the total pressure of the gases in the collection bottle is given as 760 torr. We are also given that the vapor pressure of water (PH2O) at 20.0◦C is equal to 17.5 torr.

The partial pressure of oxygen (PO2) can be calculated by subtracting the vapor pressure of water from the total pressure:

PO2 = Total pressure - Vapor pressure of water

PO2 = 760 torr - 17.5 torr
PO2 = 742.5 torr

Therefore, the partial pressure of oxygen collected by water displacement is 742.5 torr.