Trying to wrap my head around this, thanks for the help:
You have 8.63 moles of C2H6O2 in the following unbalanced equation: (I already balanced it, here is the balanced):
C2H6O2 + 5 O2 → 4 CO2 + 6 H2O
How many moles of water are produced in this reaction?
You came close but it isn't balanced.
2C2H6O2 + 5O2 ==> 4CO2 + 6H2O
mols C2H6O2 = grams/molar mass = ?
Then mols H2O = ?mols C2H6O2 x (6 mols H2O/2 mols C2H6O2) = ?mols C2H6O2 x 6/2 = ?
Sorry! My typo, I did have a 2 there.
So where I was making my mistakes was with the amount of each substance contained in the equation. (In other words, I forgot to include that it was 2 mols of H2O in the formula and divide by that amount). Thanks for the explanation!
To find out how many moles of water are produced in this reaction, we need to use the balanced equation:
C2H6O2 + 5 O2 → 4 CO2 + 6 H2O
From the balanced equation, we can see that for every 1 mole of C2H6O2, 6 moles of H2O are produced.
Therefore, to calculate the number of moles of water produced, we can use the following conversion:
(8.63 moles C2H6O2) x (6 moles H2O / 1 mole C2H6O2) = 51.78 moles H2O
So, 51.78 moles of water are produced in this reaction.