*You can find the right amount to optimize the reaction and save reactants so you don't waste money. To help you understand how astronomically big this number is if I gave everyone on Earth (estimated 7 billion) million dollars a day; I could keep handing out money for 78564 years. For solids or liquids that aren't solutions its sample mass/molecular weight=moles. For example to find one mole of lets say carbon-14 the equation is x/14=1 x=14grams Another example: Find 5 moles of H2O. First off just pick a molecule(any of them work but the biggest is usually the best) and assign it a number (again any number works but to keep it easy use one).*So far we have: C6H12O6 O2 -- H2O CO2 (1) So on the left side we have 6 carbon atoms 12 hydrogen atoms and an unknown amounts of oxygen atoms. Since we know the left sides number of carbon and hydrogen atoms we know the right sides number.

We have to balance the molecules to have the same number of atoms.

6 H2O- Since we have 12 hydrogen atoms and each molecule has 2 atoms we 6 molecules of water.

If you add up the mass for one side it should equal the sum of the mass on the other side.

If not you messed up somewhere and need to review your work.

12/2=6 oxygen molecules That is the last number we need and the equation is balanced C6H12O6 O2 -- H2O CO2 (1) (6) (6) (6) That one was really easy but sometimes you will get an equation that doesn't work out so well.

Sometimes one of the number wont come out as a whole number and that just wont work, because you can't have half of a molecule.The relationship between volume and temperature is Charles's law which is at constant pressure a given mass of gas's volume increases as a factor of its temperature. The other law is Boyle's law which shows the relationship between pressure and volume.The law states that at a constant temperature a give mass of gas's volume decreases as pressure goes up.6 H2O= 6 oxygen atoms 6 CO2= 12 oxygen atoms 6 12=18 atoms If we know the number on the right side we know the number on the left side.Since we have one molecule of sugar that needs six atoms of oxygen; we subtract six from 18.You may have noticed I said this is for solids and liquids, but I have been using gases.Theoretically you can use this for any type of stoichiometry if you know the chemical equation and the mass of one of the substances, but in practice gases are difficult to work with, so finding the mass becomes problematic.You need a different mole equation to work with gases.Stoichiometry with gases everything stays the same but the equation you use to find the moles.6 CO2- Since we have 6 carbon atoms and each molecule has one atom in it we need 6 molecules of CO2 So now the equation looks like that and we are almost done: C6H12O6 O2 -- H2O CO2 (1) x (6) (6) Now that we know the number of molecules on the right we know the number of oxygen atoms in the equation.We have six H2O molecules each with one oxygen atom, so we have 6 oxygen atoms in those molecules.

## Comments Stoichiometry Problem Solving

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