A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium.

What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.0 atm?

This is a new chapter were covering and i have no idea how to do this?

What is Keplers third Law? http://en.wikipedia.org/wiki/Kepler%27s_laws_of_planetary_motion

To calculate the partial pressure of oxygen in a heliox diving mixture, you need to use Dalton's Law of Partial Pressures. According to this law, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the individual gases.

To solve this problem, follow these steps:

1. Write down the given information:
- Oxygen (O₂) mass: 2.0 g
- Helium (He) mass: 98.0 g
- Total pressure (Pᵢ): 8.0 atm

2. Calculate the mole fraction of oxygen (Xᵢ):
- Mole fraction (Xᵢ) is the ratio of the moles of oxygen to the total moles of both gases.

The number of moles of oxygen (nᵢ) can be calculated using the oxygen mass (mᵢ) and its molar mass (Mᵢ):
nᵢ = mᵢ / Mᵢ

The number of moles of helium (nⱼ) can be found similarly:
nⱼ = mⱼ / Mⱼ

Since the ratio of moles to mass is inherently the same, Xᵢ can be calculated using this formula:
Xᵢ = nᵢ / (nᵢ + nⱼ)

3. Calculate the partial pressure of oxygen (Pᵢ) using Dalton's Law:
- The partial pressure of oxygen (Pᵢ) can be found by multiplying the mole fraction (Xᵢ) and the total pressure (P):
Pᵢ = Xᵢ * P

Now, let's perform the calculations:

1. Given information:
- mᵢ (oxygen mass) = 2.0 g
- Mᵢ (oxygen molar mass) = 32 g/mol

- mⱼ (helium mass) = 98.0 g
- Mⱼ (helium molar mass) = 4 g/mol

- P (total pressure) = 8.0 atm

2. Calculate the moles:
nᵢ = mᵢ / Mᵢ = 2.0 g / 32 g/mol = 0.0625 mol
nⱼ = mⱼ / Mⱼ = 98.0 g / 4 g/mol = 24.5 mol

3. Calculate the mole fraction:
Xᵢ = nᵢ / (nᵢ + nⱼ) = 0.0625 mol / (0.0625 mol + 24.5 mol) = 0.0025

4. Calculate the partial pressure of oxygen:
Pᵢ = Xᵢ * P = 0.0025 * 8.0 atm = 0.02 atm

Therefore, the partial pressure of oxygen in the heliox diving mixture delivered at a total pressure of 8.0 atm is 0.02 atm.

Hmmmm. How did those get posted, I was working on an astronomy question.

figure moles of O2 and He in a mixture of 1000 grams.

now add them to get total moles.

partial pressure O2 =(molesO2/totalmoles)*totalpressure