Question #5564b

1 Answer
Apr 12, 2017

The reaction will require 0.373 mol of oxygen.


First, we need to write a balanced equation for this combustion:

#C_3H_8+5O_2 rarr 3CO_2 + 4H_2O#

This equation assumes complete combustion has occured, meaning that carbon dioxide is one of the products.

Looking at the equation, we see that each one mole of propane #(C_3H_8)# that burns will require five moles of oxygen.

To solve the problem, first convert the mass of propane to moles:

#3.28 g -: 44 g/"mol" = 0.0745# mol of propane

Next, multiply this amount by 5 as given in the proportions set out in the equation:

#0.0745 xx 5 = 0.373 "mol of " O_2# required.