0.130 mol of octane is allowed to react with 0.710 mol of oxygen.
How many moles of water are produced in this reaction?
The balanced equation for the combustion of octane (C8H18) with oxygen (O2) to produce water (H2O) and carbon dioxide (CO2) is:
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
From the balanced equation, we can see that 2 moles of octane produce 18 moles of water.
Given that 0.130 mol of octane is reacting, we first need to determine the stoichiometric ratio of octane to water in the reaction.
0.130 mol octane x (18 mol water / 2 mol octane) = 0.130 mol * 18 / 2 = 1.170 mol water
Therefore, in this reaction, 1.170 moles of water are produced.