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A diver breathes a heliox mixture with an oxygen mole fraction of 0.050. What must the total pressure (in atm) be for the partial pressure of oxygen to be 0.21 atm?

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Answer:

4.2 atm

Explanation:

Dalton’s Law of Partial Pressures

PA = XA(PT)

Partial pressure of A = mole factor of gas A x total pressure of all gases

PA = 0.21 atm

XA = 0.050

PT= ?

0.21atm= 0.050(PT)

0.21/0.050 = PT

PT = 4.2 atm

samueladesida43

The total pressure of gases must be 4.2 atm for the partial pressure of oxygen to be 0.21 atm.

How to calculate partial pressure?

The partial pressure of a gas can be calculated using Dalton's law of partial pressure equation as follows:

PA = XA(PT)

Where;

  • PA = partial pressure of oxygen
  • XA = mole factor of oxygen
  • PT = total pressure of all gases

Based on the information given in this question;

  • PA = 0.21 atm
  • XA = 0.050
  • PT= ?

0.21 atm = 0.050 (PT)

0.21/0.050 = PT

PT = 4.2 atm

Therefore, the total pressure of gases must be 4.2 atm for the partial pressure of oxygen to be 0.21 atm.

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