Consider the molecular-level representation of a mixture of gases. If the partial pressure of the diatomic gas is 0.780atm, what is the total pressure?

Question

Consider the molecular-level representation of a mixture of gases. If the partial pressure of the diatomic gas is 0.780atm, what is the total pressure?

Answer 1

If this is in reference to the picture with 14 dots- green (3-diatomic), orange(5), and blue (6):

You can use this representation of the molecular level to set up a mole fraction for the diatomic gas:

Mole fraction= Number of moles/ total moles

Mole fraction_diatomic= Number of moles_diatomic/ total moles

Mole fraction_diatomic (X_diatomic)= 3 (green)/14 (total) = 0.21

Dalton's Law of Partial Pressures:

The total pressure of the mixture of gasses is the sum of the individual pressures of each gas (P_total= P₁+P₂+......)

if........... P_diatomic= P_Total • X_diatomic

then ....(P_diatomic / X_diatomic)= P_Total

You can use this representation of the molecular level to set up a mole fraction for the diatomic gas:

Mole fraction= Number of moles/ total moles

Mole fraction_diatomic= Number of moles_diatomic/ total moles

Mole fraction_diatomic (X_diatomic)= 3 (green)/14 (total) = 0.21

Dalton's Law of Partial Pressures:

The total pressure of the mixture of gasses is the sum of the individual pressures of each gas (P_total= P₁+P₂+......)

if........... P_diatomic= P_Total • X_diatomic

then ....(P_diatomic / X_diatomic)= P_Total