Chapter 11, Problem 11.69P

Interpretation Introduction

Interpretation:

The reason behind the fact that percentage yield cannot be greater than $100\%$ has to be determined. Also, the reason for percentage yield measured in lab to be greater than $100\%$ has to be explained.

Concept Introduction:

Mole is S.I. unit. The number of moles is calculated as ratio of mass of compound to molar mass of compound.

Molar mass is sum of the total mass in grams of all atoms that make up mole of particular molecule that is mass of 1 mole of compound. The S.I unit is $\text{g/mol}$.

The expression to relate number of moles, mass and molar mass of compound is as follows:

  $\text{Number of moles}=\frac{\text{mass of the compound}}{\text{molar mass of the compound}}$

Percent yield is ratio of actual yield by theoretical yield. Actual yield is amount of actual product formed in chemical reaction.

Theoretical yield is amount of product formed from reactant according to stoichiometry in the balanced chemical reaction.

The expression for percent yield is as follows:

  $\text{Percent yield}\left(\%\right)=\left(\frac{\text{actual yield}}{\text{theoreticalyield}}\right)\left(100\right)$