A bearthing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1.2 atm if PHe = 0.98 atm and PCO2 = 0.04 atm?
a) 1.02 atm
b) 0.12 atm
c) 0.94 atm
d) 0.18 atm
If you mean the total pressure is 1.2 atm, then PO2+PHe+PCO2=1.2atm
PO2+PHe+PCO2=1.2atm solve for PO2
PO2= 1.2atm-PHe-PCO2
answer is d
To find the partial pressure of oxygen, we need to subtract the partial pressures of helium and carbon dioxide from the total pressure of 1.2 atm.
Partial pressure of oxygen = Total pressure - Partial pressure of helium - Partial pressure of carbon dioxide
Partial pressure of oxygen = 1.2 atm - 0.98 atm - 0.04 atm
Partial pressure of oxygen = 0.18 atm
Therefore, the partial pressure of oxygen at 1.2 atm is 0.18 atm.
Answer: d) 0.18 atm
To find the partial pressure of oxygen in the breathing mixture, you can use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas.
In this case, the total pressure is given as 1.2 atm. We know the partial pressure of helium (PHe) is 0.98 atm and the partial pressure of carbon dioxide (PCO2) is 0.04 atm.
To find the partial pressure of oxygen (PO2), you need to subtract the sum of the partial pressures of helium and carbon dioxide from the total pressure:
PO2 = Total pressure - (PHe + PCO2)
PO2 = 1.2 atm - (0.98 atm + 0.04 atm)
PO2 = 1.2 atm - 1.02 atm
Simplifying the equation, we get:
PO2 = 0.18 atm
Therefore, the partial pressure of oxygen at 1.2 atm is 0.18 atm, which corresponds to option d) in the given choices.