Chapter 3, Problem 3.138QE

Interpretation Introduction

Interpretation:

The percent yield has to be calculated for the given reaction, if $\text{5}{\text{.0×10}}^{\text{3}}\text{g}$${\text{H}}_{\text{2}}$ reacts with excess $\text{CO}$ to form $\text{3}{\text{.5×10}}^{\text{3}}\text{g}$${\text{CH}}_{\text{3}}\text{OH}$.

  ${\text{CO}}_{\text{(g)}}{\text{ + 2H}}_{\text{2(g)}}\stackrel{}{\to }{\text{CH}}_3{\text{OH}}_{\text{(l)}}$

Concept Introduction:

The mass of a product isolated from a reaction is known as the actual yield.  The actual yield of a product, the result of a laboratory experiment is less than the theoretical yield and is expressed as percent yield.

Limiting reactant:

Limiting reactant is the one that yields the smallest amount of any one product.  If the mass of more than one reactant is given, approach the stoichiometry problem by calculating the number of moles of product formed from the quantity of each reactant.  The reactant that yields the smallest amount of product is limiting; use it for the stoichiometry calculation.