CO2 = 0.0687 atm and O2 = 0.161 atm.
To find the partial pressure of each gas, we need to use the mole fractions and total pressure given in the problem:
partial pressure of CO2 = mole fraction of CO2 x total pressure
partial pressure of O2 = mole fraction of O2 x total pressure
Plugging in the numbers, we get:
partial pressure of CO2 = 0.0998 x 0.6880 atm = 0.0687 atm
partial pressure of O2 = 0.2340 x 0.6880 atm = 0.161 atm
Therefore, the correct answer is A: CO2 = 0.0687 atm and O2 = 0.161 atm.
A special gas mixture is used in bacterial growth chambers which contains 5.00% by mass of CO2 and 95.0% O2. If the mole fraction of CO2 and O2 in the mixture is 0.0998 and 0.2340, respectively. What is the partial pressure in atmospheres of O2 and CO2 gases at a total pressure of 0.6880 atm?
CO2 = 0.0687 atm and O2 = 0.161 atm
CO2 = 0.000494 atm and O2 = 0.2223 atm
CO2 = 0.0998 atm and O2 = 0.2340 atm
CO2 = 0.6536 atm and O2 = 0.0344 atm
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