LAW OF CONSERVATION OF MASS

 

Let’s consider a simple chemical reaction involving the combustion of methane (CH₄) in oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). The balanced chemical equation for this reaction is:${\text{CH}}_4(g)+2{\text{O}}_2(g)\to {\text{CO}}_2(g)+2{\text{H}}_2\text{O}(g)$Methane + Oxygen → Carbon Dioxide + Water

Data Table for Analysis

To understand this reaction better, we can analyze the masses of the reactants and products involved:

Analysis of the Data

1. Mass of Reactants:
   • The mass of methane (CH₄) is 16 grams.
   • The mass of oxygen (O₂) is 64 grams $2\times 32\text{g/mol}<br>$
   • Therefore, the total mass of the reactants is: $16\text{g}+64\text{g}=80\text{g}$
2. Mass of Products:
   • The mass of carbon dioxide (CO₂) produced is 44 grams.
   • The mass of water (H₂O) produced is 36 grams $2\times 18\text{g/mol}<br>$
   • Therefore, the total mass of the products is: $44\text{g}+36\text{g}=80\text{g}$