A mixture containing 4.33 g of CO2 and 3.11 g of CH4 has a total pressure of 1.09 atm. What is the partial pressure of CO2 in the mixture?
Step 1 of 2
Here, we need to calculate the partial pressure of helium in the mixture.
Step1 : Dalton's law of partial pressures: It states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.
Partial pressure can be calculated by using ideal gas equation if we assume that each gas acts independently.
Therefore, From the ideal gas equation,
PV = nRT
Pn = nnRT/V………….(1)
Therefore, when a mixture contain multi component, then the partial pressure of each component would be.
Pa = naRT/V ………(2)
Pb = nbRT/V …….
Thus, total pressure P = Pa + Pb +.....
= RT/V(na + nb+.....)
Divide the equation (2) by equation (3) we get
= = na/nn ----(4)
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
Since the solution to 120P from 11 chapter was answered, more than 549 students have viewed the full step-by-step answer. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 120P from chapter: 11 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This full solution covers the following key subjects: pressure, mixture, containing, partial, atm. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “A mixture containing 4.33 g of CO2 and 3.11 g of CH4 has a total pressure of 1.09 atm. What is the partial pressure of CO2 in the mixture?” is broken down into a number of easy to follow steps, and 29 words.