Theoretical, Actual, Percent Yield & Error - Limiting Reagent and Excess Reactant That Remains

TL;DR

Learn how to calculate actual yield, theoretical yield, and percent yield through practice problems and understand the concepts of limiting reactant and excess reactant.

Transcript

in this video we're going to focus on how to calculate the actual yield the theoretical yield and the percent yield so as you can see the equation is on the board percent yield is equal to actual over theoretical times 100 now we're going to go over a few practice problems uh using that equation we're also going to talk about the difference between... Read More

Key Insights

• 🫀 Balancing a combustion reaction involves adjusting coefficients to ensure an equal number of atoms on each side.
• 🥳 The mole-to-coefficient ratio helps determine the limiting reactant in a reaction.
• ⚾ Theoretical yield represents the maximum amount of product that can be obtained based on stoichiometry.
• ❓ Actual yield is the amount of product actually obtained in an experiment, which is usually less than the theoretical yield.
• 🗂️ Percent yield indicates the efficiency of a reaction and can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100.
• ❎ Percent error measures the deviation between the theoretical and actual yields, with negative values indicating an underestimate and positive values indicating an overestimate.
• ❓ Excess reactant refers to the reactant that is not completely used up in a reaction.

Summary & Key Takeaways

• The video focuses on calculating actual yield, theoretical yield, and percent yield in chemical reactions.

• It explains the process of balancing a combustion reaction and identifying the limiting reactant.

• The video provides step-by-step calculations to find the theoretical yield and actual yield, as well as the percent yield and percent error.

• It also demonstrates how to determine the amount of excess reactant that remains after the reaction.