The measured amount of product-
The measured amount of product-
The measured amount of product.
The actual yield of a reaction product is always less than the yield from the chemical equation. This is because of error.
The actual energy change for a reaction might be different from the predicted energy change due to experimental errors, incomplete reactant conversion, side reactions, impurities in reactants, or inaccurate assumptions about reaction conditions. Kinetic factors such as reaction rates and temperature variations during the reaction can also contribute to discrepancies between predicted and actual energy changes.
(Actual yield / Theoretical yield) x 100%
Yes. That is the actual definition of an enzyme.
"Reagents" or "starting materials".
No, actual yield cannot exceed 100% in a reaction. A yield of 110% would imply that more product was obtained than theoretically possible based on stoichiometry, which is not physically possible. It usually indicates experimental error or incomplete purification of the product.
You can determine if a reaction is stoichiometric by comparing the balanced chemical equation to the actual amounts of reactants and products in the reaction. If the amounts of reactants and products are in the exact ratios as predicted by the balanced equation, then the reaction is stoichiometric.
This is usually referred to as the ACTUAL YIELD of that substance.
Theoretical= calculated
It is a chemical reaction which then shoots out like a volcano does