on a particularly hot 30 degrees C day near the seashore the partial pressure of water vapor in the air is .0303atm. given that the atmospheric pressure is 1 atm and the composition of dry air is 78% N, 21% O and 1%Ar, what is the partial pressure of oxygen gas?

To find the partial pressure of oxygen gas in the air, we need to consider the composition of dry air and the given partial pressure of water vapor.

Let's start by calculating the partial pressure of dry air components, excluding water vapor.

1. Find the partial pressure of nitrogen (N₂):
Given that dry air comprises 78% nitrogen, we can calculate its partial pressure using the atmospheric pressure (1 atm):
Partial pressure of nitrogen = 78% of 1 atm = 0.78 atm

2. Find the partial pressure of oxygen (O₂):
Similarly, dry air comprises 21% oxygen, so we can calculate its partial pressure using the atmospheric pressure:
Partial pressure of oxygen = 21% of 1 atm = 0.21 atm

3. Find the partial pressure of argon (Ar):
Dry air contains 1% argon, so we can calculate its partial pressure:
Partial pressure of argon = 1% of 1 atm = 0.01 atm

Now, to find the total pressure of dry air components, we sum up their partial pressures:
Total pressure of dry air = Partial pressure of nitrogen + Partial pressure of oxygen + Partial pressure of argon

Total pressure of dry air = 0.78 atm + 0.21 atm + 0.01 atm = 1 atm

Since the total pressure of dry air is equal to the atmospheric pressure, we know that the partial pressure of water vapor must be subtracted from the atmospheric pressure to account for its contribution.

Partial pressure of oxygen = Atmospheric pressure - Partial pressure of water vapor

Partial pressure of oxygen = 1 atm - 0.0303 atm = 0.9697 atm

Therefore, the partial pressure of oxygen gas in this given scenario is 0.9697 atm.