Define and explain the concept of percent yield... - SS1 Chemistry Redox Reactions Question

Percent yield is a measure of the efficiency of a chemical reaction and represents the ratio of the actual yield of a product to the theoretical yield, expressed as a percentage. It quantifies how much of the desired product is obtained compared to the maximum possible yield.

 

The percent yield can be calculated using the formula:

 

Percent yield = (Actual yield / Theoretical yield) x 100

 

Several factors can affect the percent yield in a chemical reaction:

 

1. Limiting reactant: The identification of the limiting reactant is crucial in determining the maximum theoretical yield. If the reaction is not carried out under ideal conditions or if the reactants are not in the exact stoichiometric ratio, the actual yield may be lower than the theoretical yield, leading to a lower percent yield.
2. Side reactions: Side reactions can occur alongside the desired reaction and result in the formation of unwanted products. These side reactions reduce the amount of the desired product and lower the percent yield.
3. Incomplete reaction: In some cases, the reaction may not go to completion due to various reasons such as reversible reactions, equilibrium conditions, or competing reactions. Incomplete reaction results in a lower actual yield and consequently a lower percent yield.
4. Purity of reactants and products: Impurities in the reactants or products can affect the yield. Impure reactants may react differently, leading to a lower yield of the desired product. Impurities in the product can also affect the accuracy of measuring the actual yield, thus affecting the percent yield.
5. Experimental errors: Errors in measurements, transfers, and calculations can introduce inaccuracies in determining the actual yield, leading to a deviation from the theoretical yield and affecting the percent yield.