## Introductory Chemistry (5th Edition)

The partial pressure of the $CO_{2}$ is 0.367 atm
We can use Dalton's Law of partial pressures to find the partial pressure the carbon dioxide gas exerts by using the mole fraction and multiplying it by the total pressure. First we must determine the number of moles of each gas by taking the quantity and dividing by the molar mass of that gas. Then we must determine the fraction of carbon dioxide gas compared to the total amount which is calculated by taking the moles of carbon dioxide divided by the total number of moles of all the gases in the mixture Moles of $CO_{2}$ = $4.33 g\div 44.01 = 0.09838673 mols CO_{2}$ Moles of $CH_{4}$ = $3.11g\div 16.04 = 0.19389027 mols CH_{4}$ Total Number of Moles; $0.09838673 + 0.19389027 =0.292277$ $CO_{2}$ Mole Fraction = $\frac{0.09838673 moles}{(0.292277 moles)} = 0.3366$ Therefore, the $Partial Pressure = 0.3366*1.09 atm = 0.367 atm$