Question
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 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?
Answers
DrBob222
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 = ?
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 = ?
BHT
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!
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!