Which law of chemical combination is illustrated by the fact that 168gFe reacts with 72gH2O to from 232gFeO4 and 8gH2?
The law of chemical combination that is illustrated by the given reaction is the law of conservation of mass. According to this law, in a chemical reaction, the mass of the reactants must be equal to the mass of the products.
To understand how this law is applied in this reaction, we need to identify the reactants and products and calculate their masses.
Given:
Mass of Fe = 168 g
Mass of H2O = 72 g
Mass of FeO4 = 232 g
Mass of H2 = 8 g
Reactants:
Fe + H2O
Products:
FeO4 + H2
To determine whether the law of conservation of mass holds true, we need to calculate the total mass of the reactants and compare it to the total mass of the products.
Total mass of reactants:
Mass of Fe + Mass of H2O = 168 g + 72 g = 240 g
Total mass of products:
Mass of FeO4 + Mass of H2 = 232 g + 8 g = 240 g
As you can see, the total mass of the reactants (240 g) is equal to the total mass of the products (240 g). Therefore, the law of conservation of mass is illustrated in this reaction. The observed masses of the reactants and products satisfy the law, demonstrating that no mass is gained or lost during the reaction.