What is the pressure in a 5.23-L flask if 0.233 mol of carbon dioxide is added to 0.469 mol of oxygen? The temperature of the mixture is 50.8 degrees C.

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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What is the pressure in a 5.23-L flask if 0.233 mol of carbon dioxide is added to 0.469 mol of oxygen? The temperature of the mixture is 50.8 degrees C.

 
Expert Solution
Step 1

GIVEN:

Moles of Carbon Dioxide= 0.233 mol

Moles of Oxygen =0.468 mol

The volume of the container= 5.23 L

Temperature= 50.8o C = 323.8 K

To Calculate: Total pressure in the flask

Step 2

According to Dalton's law of Partial Pressure, the total pressure in the flask is equal to the sum of partial pressure of the individual gases.

PT = PCO2 + PO2 

The partial pressure of CO2 can be calculated using IDEAL GAS Equation

PCO2 = nRT/V

PCO2 =0.233 mol×0.0821 L atm K-1mol-1×323.8 K5.23 LPCO2 =1.184 atm

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