Question

"How many moles of water are produced when 0.425 mole of octane burns in the

following reaction?
2C₈H₁₈(l) + 25O₂(g) → 16CO₂(g) + 18H₂O(g)

Answer 1

3.825 moles of water are produced when 0.425 mole of octane burns in the given reaction.

Step-by-step explanation:

In the given reaction:

2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(g)

It can be observed that for every 2 moles of octane (C8H18) burned, 18 moles of water (H2O) are produced.

Therefore, if 0.425 mole of octane burns, the number of moles of water produced can be calculated as follows:

0.425 mol octane x (18 mol water / 2 mol octane) = 3.825 mol water

So, 3.825 moles of water are produced when 0.425 mole of octane burns in the given reaction.