Exercise 3 | The periodic table and Chemical Periodicity
The unbalanced chemical equation of the combustion of octane is:
C8H18 (l) + O2 (g) → CO2 (g) + H2O (l)
Balance the equation.
What mass of O2 will be needed to burn 50.8 g of octane?
How many moles of water are produced?
2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (l)
According to the stoechiometry of the balanced equation:
= ⇒ = x
mO2 = 178 g
= ⇒ nH2O = x
nH2O = 4.01 mol