Butane (C4H10) burns in the presence of oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).
How many moles of water will be produced if 9.3 moles of oxygen are consumed in the reaction?
a
7.2 moles of H2O
b
9.9 moles of H2O
c
14.0 moles of H2O
d
12.1 moles of H2O
The balanced chemical equation for the combustion of butane is as follows:
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
From the balanced equation, we can see that for every 13 moles of O2 consumed, 10 moles of H2O are produced.
Therefore, if 9.3 moles of O2 are consumed, the amount of H2O produced can be calculated as follows:
(9.3 moles O2) x (10 moles H2O / 13 moles O2) = 7.15 moles H2O
So, the correct answer is:
a) 7.2 moles of H2O