0.130 mol of octane is allowed to react with 0.800 mol of oxygen.
How many moles of water are produced in this reaction?
The balanced chemical equation for the combustion of octane (C8H18) is:
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
From the balanced equation, we can see that 1 mole of octane produces 18 moles of water.
Given:
- Moles of octane (C8H18) = 0.130 mol
- Moles of oxygen (O2) = 0.800 mol
Since octane is the limiting reactant, all 0.130 mol of octane will react. This will produce 18 moles of water for every 2 moles of octane. Therefore, the number of moles of water produced will be:
0.130 mol octane * (18 mol water / 2 mol octane) = 1.17 mol water
So, 1.17 moles of water are produced in this reaction.