A gaseous mixture containing 1.5 mol of Ar and 3.5 mol of CO2 has a total pressure of 7.0 atm . What is the partial pressure of CO2.

4.9 atm

Explanation:

Given:

Total pressure = 7.0 atm

(Total number of moles)=[ (1.5 mol arg) + (3.5 mol co2) ]

= 5 moles

Let Partial pressure of CO2 gas = P(CO2)

✓✓partial pressure of CO2 can be calculated using below expresion.

P(CO2) / Total pressure = (moles of CO2 gas) / Total number of moles

✓✓ Let us substitute the values into the above expresion.

[P(CO2) / 7.0 atm ] = [3.5 mol / 5 moles]

P(CO2)= [7 atm × 3.5 moles] / [5 moles]

= 4.9 atm

Hence, the partial pressure of CO2 is 4.9 atm

Partial pressure of CO₂ = 4.9 atm

Explanation:

From the question given above, the following data were obtained:

Mole of Ar = 1.5 moles

Mole of CO₂ = 3.5 moles

Total pressure (Pₜ) = 7.0 atm

Partial pressure of CO₂ =?

Next, we shall determine the mole fraction of CO2. This can be obtained as follow:

Mole of Ar = 1.5 moles

Mole of CO₂ = 3.5 moles

Total mole = 1.5 + 3.5

Total mole = 5 mole

Mole fraction of CO₂ = mole of CO₂ / total mole

Mole fraction of CO₂ = 3.5 / 5

Mole fraction of CO₂ = 0.7

Finally, we shall determine the partial pressure of CO₂. This can be obtained as follow:

Total pressure (Pₜ) = 7.0 atm

Mole fraction of CO₂ = 0.7

Partial pressure of CO₂ =?

Partial pressure of CO₂ = mole fraction of CO₂ × total pressure

Partial pressure of CO₂ = 0.7 × 7

Partial pressure of CO₂ = 4.9 atm

it is the most commonly accepted one

it’s previous models   because when i picked that son of a gun’s answer it was wrong look for previous models because they might make it a different letter