🤓 Based on our data, we think this question is relevant for Professor Blankenship's class at UGA.
Recall: Dalton’s Law of Partial Pressures states that the total pressure of a mixture of unreacting gases is the sum of the partial pressures of the individual gases.
The partial pressure of a gas in the mixture is the product of the total pressure of the mixture and the mole fraction, χ, of the gas:
We first need to calculate the mole fraction of the gases before calculating their partial pressures. The molar mass of O2 is 2(16.00 g/mol O) = 32.00 g/mol and the molar mass of CO2 is 12.01 g/mol C + 2(16.00 g/mol O) = 44.01 g/mol.
A tank contains a mixture of 52.5 g oxygen gas and 65.1 g carbon dioxide gas at 27°C. The total pressure in the tank is 9.21 atm. Calculate the partial pressures of each gas in the container.
Frequently Asked Questions
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 Partial Pressure concept. You can view video lessons to learn Partial Pressure. Or if you need more Partial Pressure practice, you can also practice Partial Pressure practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Blankenship's class at UGA.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.