0
When calculating the theoretical yield of a product within a reaction, the idea is to convert mass reactant --> mass product; in other words, "how many grams of product X will N grams reactant A and N grams reactant B yield (create)?" Whichever mass is the lowest is considered the theoretical yield (in other words, the reactant that produces the least amount of product).
__A + __B --> __X
mass reactant A => mass product X (mass A: mass X)
mass reactant B => mass product X (mass B: mass X)
In order to calculate the theoretical yield, you need to convert the mass of reactant A to the mass of product X AND the mass of reactant B to the mass of product X.
1. Multiply the mass of the reactant by the number of molecules (or moles) X and by the molar mass of X.
2. Divide the above by the molar mass of reactant (which is multiplied by the number of molecules [or moles] of reactant).
Do this for each reactant involved.
- Formula
Mass reactant * # molecules (moles) product X1 * molar mass product X
--------- # molecules (moles) reactant * molar mass reactant
= Mass Product X
- Conversion Factor
Mass reactant * 1 mol reactant * # molecules product X * molar mass product X
-------------- molar mass reactant - # molecules reactant --- 1 mol product X
= Mass Product X
1the # molecules is obtained from the balanced equation. For clarification, I stated # molecules in place of mol; however, on practice problems and in textbook tutorials on how to solve problems in regards to stoichiometry, it is likely it will say mol or moles instead of # molecules.
Ex. Ca(NO3)2 + 2NaF --> CaF2 + 2NaNO3
What is the theoretical yield of CaF2 (product X) when 43.5g Ca(NO3)2 (reactant A) react with 39.5g NaF (reactant B)?
43.5g Ca(NO3)2 * 1 mol Ca(NO3)2 * 1 molecule1 CaF2 * 78.08g CaF2
-------------- 164.1g Ca(NO3)2 ----- 1 molecule1 Ca(NO3)2 - 1 mol NaF
= 22.3g CaF2
36.5g NaF * 1 mol NaF * 1 molecule1 CaF2 * 78.08g CaF2
------------ 41.99g NaF --- 2 molecules1 NaF --- 1 mol CaF2
= 36.7g CaF2
The theoretical yield of CaF2 is 22.3g, as it is the lowest amount of product created. In this case, the limiting reagent (the reactant that produced the least product) is Ca(NO3)2 and the reagent in excess is NaF.
"A chain is only as strong as its weakest link".
What else can I help you with?
Is Time a Spacial Dimention?
Yes. Time and Space are the same thing, only in different forms. Theoretical physicists have done the math, and calculate that there should be around 10 dimensions in our space.
What is the largest nuclear bomb?
The Tsar Bomba. It was tested in 1961 by the USSR on the island of Novaya Zemlya within the Arctic Circle. Its design yield was 100 megatons, but the yield was reduced to 57 megatons for the test by replacing the uranium-238 third stage tamper with a different metal (e.g. lead, tungsten) that would not fission when hit by the high energy fusion neutrons (and thus would not contribute to the yield or the fallout).The Tsar Bomba was not only the highest yield nuclear bomb ever tested, it was the highest yield nuclear bomb actually dropped from a bomber airplane. The Tsar Bomba also turned out to be the cleanest nuclear explosion with only about 3% fission yield and a correspondingly small amount of fallout relative to its total yield. Nuclear explosions having 5% or less fission yield are usually called "clean".
What is the name for the level of crop ouput from a given level of input?
That would be the yield.
What is the name for the theoretical end-product gravitational collapse of a massive star?
impload
The French sociologist who is described as the founding figure of the functionalist theoretical tradition is?
Emile Durkheim
HOW TO calculate percentage yield?
actual yield multiply by 100 = % yield theoretical yield
What is the percent yield for the reaction below when 544.5 g SO2 and 160.0 g O2 produce 382.0 g SO3?
Percent yield = (actual yield ÷ theoretical yield) × 100% Calculate the moles of SO2 and O2 used, then determine the limiting reactant. From the limiting reactant, calculate the theoretical yield of SO3. Compare the actual yield to the theoretical yield to calculate the percent yield.
How calculate the percantage yield in balanced chemical equation?
To calculate the percentage yield in a balanced chemical equation, you first need to determine the theoretical yield (the maximum amount of product that can be formed based on stoichiometry). Then, measure the actual yield produced in the lab experiment. Divide the actual yield by the theoretical yield, and then multiply by 100 to get the percentage yield. The formula is: (actual yield / theoretical yield) x 100%.
The actual yield of the given reaction is 14.4what is your percent yield?
To calculate percent yield, you would use the formula: (actual yield / theoretical yield) * 100%. If the actual yield is 14.4 and the theoretical yield is not provided, the percent yield cannot be calculated accurately without the theoretical yield.
What is the percent yield if the actual yield from this reaction is 306g?
To calculate the percent yield, you need the theoretical yield of the reaction. The percent yield is calculated using the formula: [ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 ] If you provide the theoretical yield, I can help you determine the percent yield.
What if i don't know the yield percent?
Do you need it? Are you being told to calculate it? percent yield = (actual yield) divided by (theoretical yield) x 100
How do you calculate predictions?
The theoretical yield is determinef by the study of the chemical reaction involved.
How do you calculate percentage yield?
# Determine the limiting reagent; # Calculate the expected yield if the reaction goes to 100% completion. # Divide the actual yield by the expected yield and multiply by 100. The result is percentage yield.
When 50.9 g of silicon dioxide is heated with an excess of carbon 32.3 g of silicon carbide is produced SiO2 plus 3C ----- SiC plus 2CO what is the percent yield of this reaction?
To calculate percent yield, we need to compare the actual yield to the theoretical yield. The actual yield is the measured amount of product produced, which is 32.3 g of silicon carbide. The theoretical yield can be calculated by stoichiometry. Convert 50.9g of SiO2 to moles, determine the limiting reactant, and calculate the theoretical yield of SiC. Finally, using the formula: percent yield = (actual yield / theoretical yield) * 100, we find the percent yield.
If 15.4 g of CO2 was produced from the thermal decomposition of 39.37 g of CaCO3 then what is the percentage yield of the reaction?
To find the percentage yield, you first need to calculate the theoretical yield of CO2 that would be obtained from the given mass of CaCO3. Then divide the actual yield of CO2 (15.4 g) by the theoretical yield, and multiply by 100 to get the percentage yield. The percentage yield is calculated as (actual yield / theoretical yield) * 100.
In Part A we saw that the theoretical yield of aluminum oxide is 1.70 mol . Calculate the percent yield if the actual yield of aluminum oxide is 1.24 mol .?
Percent yield is calculated by dividing the actual yield by the theoretical yield, and then multiplying by 100. In this case, the percent yield would be: (1.24 mol / 1.70 mol) * 100 = 73%. This means that 73% of the theoretical yield was obtained in the experiment.
Copper dissolves in nitric acid producing copper nitrate After a reaction with sodium hydroxide and heating copper nitrate changed to copper oxide Calculate the percent yield?
To calculate the percent yield, you need to know the amount of copper oxide formed and compare it to the theoretical yield. The theoretical yield can be calculated based on the initial amount of copper, assuming complete conversion. Once you have both values, use the formula: Percent Yield = (Actual Yield / Theoretical Yield) x 100.
