Chapter 4, Problem 4.18PAE

xInterpretation:

The gas (CH₄ or C₂H₆) that produces 1.80 g of water when 1.00 -g of this gas is combusted in excess O₂ has to be determined. Assuming complete combustion.

Interpretation Introduction

Concept Introduction:

➣ The combustion reaction is a reaction where the oxygen reacts with a compound formed by carbon and hydrogen. Its products are carbon dioxide and water when the combustion is complete.

➣ The molecular weight (MW) can be defined in the following way,

$\text{MW=}{\displaystyle \sum {\text{n}}_{\text{i}}}{\text{A}}_{\text{i}}$

  Where n_i is the number of atoms of element i that form the molecule and A_i is the atomic weight of element i.

➣ The stoichiometric coefficients show the reactants proportions that are transformed and the products proportions that are produced.

➣ The molar ratio can be used to relate:

• The moles of product formed from of certain moles of reactant.
• The moles of reactant needed to form certain moles of a product.
• The moles of a reactant needed to react with certain moles of a second reactant.