If 4.74 g of propane is allowed to completely combust, calculate the mass of carbon dioxide formed at the end. Remember the units

14.2g

Explanation:

The reaction expression is given as:

        C₃H₈  +  5O₂ → 3CO₂ + 4H₂O

Given mass of propane combusted;

   4.74g

Unknown:

Mass of carbon dioxide produced  = ?

Solution:

To solve this problem, we find the number of moles of the given propane;

   Number of moles  =  

Molar mass of C₃H₈ = 3(12) + 8(1) = 44g/mol

   Number of moles  =  = 0.11mol

From the balanced reaction equation:

          1 mole of C₃H₈ will produce  3 moles of CO₂

          0.11mole of C₃H₈ will produce 3 x 0.11  = 0.33mole of  CO₂

Mass of  CO₂ = number of moles x molar mass

    Molar mass of  CO₂ = 12 + 2(16) = 44g/mol

Mass of  CO₂ = 0.33 x 44  = 14.2g

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa