PROBLEM 27P

Consider the unbalanced equation for the combustion of butane:

C4H10(g) + O2(g) → CO2(g) + H2O(g)

Balance the equation and determine how many moles of O2 are required to react completely with 4.9 mol of C4H10

Solution 27P

Given unbalanced equation for the combustion of butane:

C4H10(g) + O2(g) → CO2(g) + H2O(g)

The balanced equation is as follows :

2C4H10 + 13O2 = 8CO2 + 10H2O

Now let’s determine how many moles of O2 are required to react completely with 4.9 mol of C4H10 :

The equation is in the ratio :

2 : 3 → 8 : 10

C4H10 : O2 is in the ratio of 2:13.

Since it only asks for the reactant side, we can cross out the product's side for now.

= 2C6H14(g)+13O2(g)

= 4.9...