Question

what is the partial pressure of carbon dioxide in a container that holds .5 moles of carbon dioxide,.32 moles of nitrogen, .2 moles of hydrogen, and has a total pressure of 1.05 atm?

Answer 1

0.58 atm

Step-by-step explanation:

Answer 2

Answer: 0.5 atm

Explanation: To calculate the partial pressure of carbon dioxide, we need to use the mole fraction of carbon dioxide and the total pressure of the container.

The mole fraction of carbon dioxide is:

X(CO2) = n(CO2) / n(total)

X(CO2) = 0.5 moles / (0.5 moles + 0.32 moles + 0.2 moles)

X(CO2) = 0.4762

The partial pressure of carbon dioxide is:

P(CO2) = X(CO2) * P(total)

P(CO2) = 0.4762 * 1.05 atm

P(CO2) = 0.5 atm (rounded to one decimal place)

Therefore, the partial pressure of carbon dioxide in the container is 0.5 atm.