Question

If a mixture of gases contains 4.5 atm of O2 and 785 mm Hg of N2. What is the total
pressure of the mixture in atm?

Answer 1

Answer:

The total pressure of the mixture is 5, 53 atm.

Explanation:

The sum of the partial pressures of the gases that make up a gaseous mixture is equal to the total pressure of said mixture, according to Dalton's law. We convert the unit of pressure in mmHg into atm:

760 mmHg----1 atm

785 mmHg----x= (785 mmHgx 1 atm)/760 mmHg=1, 03 atm

P total= P 02 + P N2

P total= 4, 5 atm + 1,03 atm=5, 53 atm

Answer 2

Contains The total pressure of the mixture is = 5, 53 atm.

What is the Mixture in the atm?

When The totality of the partial pressures of the gases that make up a gaseous mixture is equal to the total intimidation of the said mixture, according to Dalton's law. We transform the unit of pressure in mmHg into atm:

Then 760 mmHg----1 atm

After that, 785 mmHg----x= (785 mmHgx 1 atm)/760 mmHg=1, 03 atm

Now, P total is = P 02 + P N2

Therefore, P total is = 4, 5 atm + 1,03 atm=5, 53 atm

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