Hydrogen sulfide is composed of two elements: hydrogen and sulfur. In an experiment, 6.500 g of hydrogen sulfide is fully decomposed into its elements. b. What fundamental law does this experiment demonstrate?

Verified step by step guidance

1. Identify the law related to the conservation of mass in chemical reactions. This law states that mass is neither created nor destroyed in a chemical reaction.
2. Understand that when hydrogen sulfide (H2S) decomposes, it breaks down into hydrogen (H2) and sulfur (S).
3. Recognize that the total mass of hydrogen and sulfur obtained from the decomposition must equal the original mass of hydrogen sulfide used in the experiment, which is 6.500 g.
4. Consider how this experiment demonstrates the law by showing that the sum of the masses of the products (hydrogen and sulfur) equals the mass of the reactant (hydrogen sulfide).
5. Conclude that the experiment demonstrates the Law of Conservation of Mass.

Key Concepts

Law of Conservation of Mass

The Law of Conservation of Mass states that mass is neither created nor destroyed in a chemical reaction. In the context of the decomposition of hydrogen sulfide, this law implies that the total mass of the reactants (hydrogen sulfide) will equal the total mass of the products (hydrogen and sulfur) after the reaction. This principle is fundamental in understanding chemical reactions and stoichiometry.

Law of Definite Proportions

The Law of Definite Proportions asserts that a chemical compound always contains its component elements in fixed ratio by mass. In the case of hydrogen sulfide, regardless of the amount decomposed, the ratio of hydrogen to sulfur will always be the same, reflecting the consistent composition of the compound. This law is crucial for understanding the nature of chemical compounds.

Chemical Decomposition

Chemical decomposition is a process where a single compound breaks down into two or more simpler substances, often elements. In this experiment, hydrogen sulfide decomposes into hydrogen and sulfur gas. Understanding this concept is essential for analyzing reactions and predicting the products formed during chemical changes.