Problem: A mixture consisting of 7.0 g of CO and 10.0 g of SO 2, two atmospheric pollutants, has a pressure of 0.33 atm when placed in a sealed container. What is the partial pressure of CO?

FREE Expert Solution

Recall: Dalton’s law states that the total pressure of a mixture of unreacting gases is the sum of the partial pressures of the component gases.

The partial pressure of a gas in the mixture is the product of the total pressure of the mixture and the mole fraction of the gas:

We're given the mass of CO and SO2 and the total pressure of the mixture. We first need to calculate the mole fraction of CO and then we can calculate the partial pressure of CO.

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Problem Details

A mixture consisting of 7.0 g of CO and 10.0 g of SO 2, two atmospheric pollutants, has a pressure of 0.33 atm when placed in a sealed container. What is the partial pressure of CO?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.