At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
@Australopithecus @Australopithecus @Australopithecus
I block mass taggers. Sorry.
np haha i really need help on this
hi, do you have any example that you want to work or you need general idea about the topic?
i need to know the steps and a breakdown of a calculation
and HIIII @TheSmartOne!!
There are a lot of resources online... http://www.sparknotes.com/chemistry/stoichiometry/realworldreactions/section2.rhtml https://www.chem.tamu.edu/class/majors/tutorialnotefiles/limiting.htm https://www.khanacademy.org/science/chemistry/chemical-reactions-stoichiome/limiting-reagent-stoichiometry/v/stoichiometry-limiting-reagent https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/mass-relationships-and-chemical-equations-3/reaction-stoichiometry-44/calculating-theoretical-and-percent-yield-234-4704/
i need real help! i tried several sites but it didn't help me understand
by "real help" i mean personal human help
Well, it would help you to have a question so someone could help you go over it :p
okay, 02+H2 yields H2O
to calculate percent yield you need to know the theoretical yield and the real yield. Not all the reactions works 100% efficient, then if a reaction that you theoretically calculate that is going to produce 2kg of a product is only 80% efficient you are not going to get the 2 kg but the 80% of 2Kg that is going to be 1.6kg in formulas percent yield = 100 x real yield/ theoretical yield %yield = 100 x 1.6 kg/2.0 kg = 80%
the limiting reactant is the reactant in the reaction that is in lowest amount to react and the one that is going to determine the theoretical yield of the reaction. for example if you reaction after balance is 02+2H2 -> 2 H2O means that you need one mole of O2 to react with 2 moles of H2 to produce 2 moles of H2O then if you have 3 moles of O2 you will need 6 moles of H2 to produce 6 moles of H2O Now if you have the 3 moles of O2 but only 3 moles of H2 how many moles of H2O you will be able to produce? What is going to be the limiting reactant? (the reactant that is in lowest amount)
Whenever you have a reaction, to calculate the limiting reactant first you have to balance the equation and find out the stoichiometry of the reaction. Based in the stoichiometry or the proportion of combinations of the compounds you will be able to calculate how much of one or the other reactants you will need. Remember the stoichiometry is the relationship in "moles" of the different components in the chemical reaction. If you have the information in grams or liters, you have to convert them to moles to be able to calculate the relationship of combination