#theoretical yield

[er-cryptid]

Patreon | Ko-fi

[super-sarah-taylor]

Theoretical yield calculator is the best tool to determine the exact efficiency of the Chemical reaction. Learn how to calculate theoretical yield easily.

[ghcstxbcy]

hey if anyone is good at chemistry and would like to explain how the hell to find theoretical yield that'd be awesome. I have that one mole of copper (II) sulfate (3.996g) and one mole of iron (1.066g) make x grams of copper (one mole) (and then there's one mole of iron (II) sulfate but that part isn't what i need to calculate) if that helps

[elephantseltzer]

I just figured out Theoretical Yield

(molar mass)/(actual mass)X(ratio from balance equation)=limiting reactant(one of them will)

(limiting reactant)x(molar mass of product)=Theoretical Yield

In the case of a percent given use the percent as a decimal for the corresponding compound instead of a ratio.

[daysfullofdreams]

help I haven't done grade 11 chemistry for two years how do you find the theoretical yield, actual yield and percentage yield?!

[ichbinkait]

if anyone out there likes me 

or values my friendship

or any of that stuff

they will kill me so i don't have to write my chem exam tomorrow

please

anyone　

[destrucshann]

Theoretical Yield, Actual Yield, Percent Yield (in detail)

So, I know this is probably late, but I get questions (that I've ignored, lol sorry) about this a lot. And I guess it's also good to keep this here for future references, so here:

Theoretical yield is the part of the data that is calculated if/ when the experiment reaches its full capability. Usually, the theoretical yield is bigger than the actual yield. An example would be finding the mass of HCl if given 5g of H and 10g of Cl are added together. In order to find the theoretical yield, a balanced reaction is required. Then, find the limiting reactant by performing Stoichiometry. The reactant that produces the least number of the product is your limiting reactant and the amount you get from the limiting reactant is your theoretical yield.

Example:

   Balanced reaction

H2 + Cl2 = 2HCl

   Limiting reactant

5g H * 2 mol HCl  * 18g HCl = 180g HCl

(10g Cl * 2 mol HCl * 18g HCl) / 17g Cl = 21.18g HCl

Actual yield is the part of the data that is achieved after actually doing the experiment.  You can't calculate actual yield unless you perform algebra with it being "x". It is either given or obtained physically through an experiment. It is also usually less than the theoretical yield. In this case, let us pretend that the actual yield is 20.16g since I didn't do an experiment.   

Percent yield is achieved when you take the actual yield, divide it by the theoretical yield, and then multiply the answer by 100. The higher the percent yield, the better the results of your experiment.

Example:

Percent yield:

20.16g HCl / 21.18g HCl = .95g HCl * 100 = 95% HCl acquired

[jessicaauendoeschemistry-blog]

When limestone (which is principally CaCO3)is heated, carbon dioxide and quicklime (CaO) are produced by the reaction:CaCO3(s)→CaO(s) + CO2(g) .If 16.5 g of CO2 was produced from the thermal decomposition of 43.23 g of CaCO3, what is the percentage yield of the reaction?Answer in units of %.The reaction of 5.3 grams of chlorine withexcess fluorine produced 11.6 grams of ClF3.What percent yield of ClF3 was obtained?Answer in units of %.

Well it's great that you were given a balanced equation to begin with. That always helps. From there, you want to calculate the theoretical yield of CO2 produced. You do this by seeing what the maximum amount of CO2 produced from your given amount of reactant is. You must use a mole-to-mole ratio to find this equivalence. In fact, whenever you compare amounts of any two chemicals (whether they be product to product, reactant to reactant, product to reactant) you will ALWAYS use a mole to mole ratio. Don't forget this on your midterm! Here's how to do the work:

Once you know the theoretical yield (this is what you would get if you got a 100% yield, which almost never happens in real lab situations), you compare it to your actual yield by the following equation:

For the next problem, you need to write a balanced equation. It is very important to remember that in nature, Chlorine and Fluorine are both diatomic molecules. there are seven elements that behave this way: Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, and Chlorine. Remember the word "HOFBrINCl" It sounds like "Hof-brinckle". It's silly, but it works. So here is your balanced equation:

Then do as we did above and find theoretical yield.

Andddd now compare to your actual yield, which was given.