Question 8 1 pts
A closed flask contains a 0.25 moles of O2 which exerts a pressure of
0.50 atm. If 0.75 moles of CO, is added to the container what is the
total pressure in the flask?

The pressure of the closed flask after the addition of 0.75 moles of CO has been 2 atm.

Partial pressure can be defined as the pressure exerted by each gas in a given solution.

The total moles of gas in the container by the addition of CO has been:

Total moles = moles of oxygen + moles of CO

Total moles = 0.25 + 0.75

Total moles = 1 mol.

By using Dalton's law of partial pressure:

Total pressure = total moles

Total pressure = 1

Total pressure = 2 atm.

The pressure of the closed flask after the addition of 0.75 moles of CO has been 2 atm.

For more information about partial pressure, refer to the link:

link

\large \boxed{\text{2.0 atm}}  

Explanation:

We can use Dalton's Law of Partial Pressures:

Each gas in a mixture of gases exerts its pressure separately from the other gases.

0.25 mol of O₂ exerts 0.50 atm.

If you add 0.75 mol of CO, the total amount of gas is  

0.25 mol + 0.75 mol = 1.00 mol

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