If 2.70 L of propane at 24°C and 57.2 kPa is completely burned in excess oxygen, how many moles of carbon dioxide will be produced?

Stoichiometry

The answer to your question is 0.186 moles  of CO₂

Step-by-step explanation:

Data

Volume = 2.7 L

Temperature = 24°C

Pressure = 57.2 kPa

moles of CO₂ = ?

Process

1.- Calculate the moles of Propane, use the ideal gas formula

          PV = nRT

          n = PV / RT

- Convert temperature to °K          

  °K = 273 + 24 = 297

- Convert pressure to atm

          1 atm 101325 Pa

          x        57200 Pa

          x = (57200 x 1)/101325

          x = 0.56 atm

- Substitution

         n = (0.56)(2.7) / (0.082)(297)

- Simplification  

          n = 1.512 / 24.354

- Result

          n = 0.062 moles

2.- Balanced the chemical reaction

                  C₃H₈  +  5O₂   ⇒    3CO₂  +  4H₂O

3.- Calculate the moles of Carbon dioxide

                 1 moles of C₃H₈   3 moles of CO₂

                 0.062 moles         x

                 x = (0.062 x 3) / 1

                x = 0.186 moles