DEFINED AND MULTIPLE PROPORTIONS
Jess Jinete Sierra. Julia Pérez Pélez. Luis Lazcano Pacheco. Maria Fernanda Oñate.
Professor: Wilman Cabrera Lafaurie. Group: 12
Chemistry I Laboratory, Universidad del Atlántico, Barranquilla Structure | Theoretical
framework | Calculations | Analysis | Conclusions | Final | | 1 pt | 1 pt | 1.25 pt | 1.25 pt | 0.5
pt | | |
Abstract
Through the application of heat in potassium chlorate (KClO3) and potassium perchlorate
(KClO4) and applying various stoichiometric calculations in conjunction with the law of
multiple and defined proportions, we can estimate the experimental data of the composition,
quantity and relation of the reactants and the products in a chemical reaction.
Key words Laws, proportions, relation, heat
1. Introduction:
For the development of this experiment, basic knowledge of multiple proportions is needed,
which is when two elements react in more than one proportion to form different compounds,
the weights of one of the elements that combine with a fixed amount of another are in a ratio
of small whole numbers. Also, the law of definite proportions states that different samples of
the same substance contain the same elements in the same proportions.
Furthermore, we must know the concepts or methods of balancing equations by trial and
error, redox, ion-electron, among others. Together with the knowledge of what the reactant
is, what type of reaction it is, if it involves other factors (catalysts), and whether the laws
proposed in the laboratory guide are met or not.
2. Theoretical Foundations:
The Law of Definite Proportions states that different samples of the same substance contain
the same elements in the same proportions. This Law is not universal, as it does not apply to
some compounds. It was formulated by J.L. Proust and defined by John Dalton due to its
relationship with atomic theory.
The Law of Multiple Proportions was formulated by Dalton and refers to the relationship that
exists between elements that combine in more than one proportion to form different
compounds, which is obtained by varying the reaction conditions. It states: When two
elements react in more than one proportion to form different compounds, the weights of one
of the elements that combine with a fixed amount of another are in a ratio of small whole
numbers.
3. Experimental Development:
For Potassium Chlorate:
A clean and dry test tube is weighed, and between 1 and 2 g of Potassium Chlorate should
be added, taking care not to adhere it to the walls of the tube. Then, the tube is heated
gently and uniformly by rotating it in the flame, until the salt has melted, then heated strongly
until all the oxygen has been completely released. To know this, it is necessary to place a
Jess Jinete Sierra. Julia Pérez Pélez. Luis Lazcano Pacheco. Maria Fernanda Oñate.
Professor: Wilman Cabrera Lafaurie. Group: 12
Chemistry I Laboratory, Universidad del Atlántico, Barranquilla Structure | Theoretical
framework | Calculations | Analysis | Conclusions | Final | | 1 pt | 1 pt | 1.25 pt | 1.25 pt | 0.5
pt | | |
Abstract
Through the application of heat in potassium chlorate (KClO3) and potassium perchlorate
(KClO4) and applying various stoichiometric calculations in conjunction with the law of
multiple and defined proportions, we can estimate the experimental data of the composition,
quantity and relation of the reactants and the products in a chemical reaction.
Key words Laws, proportions, relation, heat
1. Introduction:
For the development of this experiment, basic knowledge of multiple proportions is needed,
which is when two elements react in more than one proportion to form different compounds,
the weights of one of the elements that combine with a fixed amount of another are in a ratio
of small whole numbers. Also, the law of definite proportions states that different samples of
the same substance contain the same elements in the same proportions.
Furthermore, we must know the concepts or methods of balancing equations by trial and
error, redox, ion-electron, among others. Together with the knowledge of what the reactant
is, what type of reaction it is, if it involves other factors (catalysts), and whether the laws
proposed in the laboratory guide are met or not.
2. Theoretical Foundations:
The Law of Definite Proportions states that different samples of the same substance contain
the same elements in the same proportions. This Law is not universal, as it does not apply to
some compounds. It was formulated by J.L. Proust and defined by John Dalton due to its
relationship with atomic theory.
The Law of Multiple Proportions was formulated by Dalton and refers to the relationship that
exists between elements that combine in more than one proportion to form different
compounds, which is obtained by varying the reaction conditions. It states: When two
elements react in more than one proportion to form different compounds, the weights of one
of the elements that combine with a fixed amount of another are in a ratio of small whole
numbers.
3. Experimental Development:
For Potassium Chlorate:
A clean and dry test tube is weighed, and between 1 and 2 g of Potassium Chlorate should
be added, taking care not to adhere it to the walls of the tube. Then, the tube is heated
gently and uniformly by rotating it in the flame, until the salt has melted, then heated strongly
until all the oxygen has been completely released. To know this, it is necessary to place a
