Chapter 9, Problem 9.51UTC

Interpretation Introduction

(a)

Interpretation:

The balanced chemical equation for the reaction should be determined.

Concept Introduction:

The balance equation for any chemical reaction represents the molecules of reactant and products with same number of atoms at both sides of the equation. The reactant and product molecules must be shown with simplest whole number coefficients.

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

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

Interpretation Introduction

(b)

Interpretation:

The percent yield of the reaction should be calculated.

Concept Introduction:

The balance equation for any chemical reaction represents the molecules of reactant and products with same number of atoms at both sides of the equation. The reactant and product molecules must be shown with simplest whole number coefficients.

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

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