Final answer:
To calculate the moles of water produced by the reaction of 1.50 moles of octane, you multiply 1.50 moles of octane by the mole ratio from the balanced chemical equation, which gives 13.5 moles of water.
Step-by-step explanation:
To find out how many moles of water are produced by the reaction of 1.50 moles of octane, we need to use the balanced chemical equation for the combustion of octane, which is represented as:
C8H18(l) + 12.5 O2(g) → 8 CO2(g) + 9 H2O(g)
From the balanced equation, we can see that 1 mole of octane produces 9 moles of water. Thus, if we have 1.50 moles of octane, we can set up a simple proportion:
1 mole of C8H18 : 9 moles of H2O
1.50 moles of C8H18 : x moles of H2O
To solve for x, we multiply 1.50 moles of octane by the mole ratio (9 moles of water per mole of octane), which gives us:
x = 1.50 moles of C8H18 × (9 moles of H2O / 1 mole of C8H18) = 13.5 moles of H2O