Question

What’s the partial pressure of carbon dioxide in a container that holds 5.0 moles of carbon dioxide, 3.0 moles of nitrogen, and 1.0 mole of hydrogen and has a total pressure of 1.05 atm? (hint: you can figure out what % of the sample is CO2 then relate that to the total pressure of the sample)

Answer 1

[AI-generated answer — Bot GPT 3.5]

To find the partial pressure of carbon dioxide, you first need to calculate the total moles of gas in the container:

Total moles of gas = 5.0 moles CO2 + 3.0 moles N2 + 1.0 moles H2
Total moles of gas = 9.0 moles

Next, calculate the % of carbon dioxide in the sample:

% CO2 = (5.0 moles CO2 / 9.0 moles total) x 100
% CO2 = 55.56%

Now, calculate the partial pressure of carbon dioxide using the % of CO2 and the total pressure of the sample:

Partial pressure of CO2 = % CO2 x Total pressure
Partial pressure of CO2 = 55.56% x 1.05 atm
Partial pressure of CO2 = 0.5556 x 1.05 atm
Partial pressure of CO2 = 0.5828 atm

Therefore, the partial pressure of carbon dioxide in the container is 0.58 atm.