Chapter 11.4, Problem 32SSC

Interpretation Introduction

Interpretation:

The reason of difference in the actual yield from a chemical reaction to the theoretical yield needs to be determined.

Concept introduction:

The actual yield of the product is the amount of product, which form at the end of reaction experimentally whereas theoretical yield represents the amount of product calculated by expecting that 100 % of reactant change to product. The percent yield can be shown as:

$\text{Percent yield = }\frac{\text{Actual yield}}{\text{Theoretical yield}}\text{ x 100}$

Answer to Problem 32SSC

• Mechanical loss of product while collecting the product.
• Formation of side products.
• Impurities in reactant.

Explanation of Solution

Given information:

There are different types of yield like theoretical yield, actual yield and percent yield

Theoretical yield is the amount of product formed according to the balance chemical reaction from the given moles and mass of reactant molecules. Actual yield is usually little lesser than the theoretical yield due to unavoidable process errors. Some of the common reasons of difference between these yields are:

• Mechanical loss of product while collecting the product.
• Formation of side products.
• Impurities in reactant.

Conclusion

Thus,

• Mechanical loss of product while collecting the product.
• Formation of side products.
• Impurities in reactant.