Ch.2 - Atoms, Molecules, and Ions

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook

Brown 15th Edition

Ch.2 - Atoms, Molecules, and Ions

Problem 12b

Chapter 2, Problem 12b

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

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.

Understand that when hydrogen sulfide (H2S) decomposes, it breaks down into hydrogen (H2) and sulfur (S).

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.

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).

Conclude that the experiment demonstrates the Law of Conservation of Mass.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

Recommended video:

Guided course

03:37

Chemical Properties

Related Practice

Textbook Question

A chemist finds that 30.82 g of nitrogen will react with 17.60, 35.20, 70.40, or 88.00 g of oxygen to form four different compounds. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 70.40 g O

371

views

Textbook Question

In the Millikan oil-drop experiment (see Figure 2.5), the tiny oil drops are observed through the viewing lens as rising, stationary, or falling, as shown here. The arrows indicate the rate of motion. a. What causes their rate of fall to vary from their rate in the absence of an electric field?

views

Textbook Question

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed into its elements, yielding 0.273 g of carbon and 0.727 g of oxygen. (a) What is the ratio of the mass of O to C?

The following diagram represents an ionic compound in which the red spheres represent cations and the blue spheres represent anions. Which of the following compounds is consistent with the drawing?

a. potassium bromide

b. potassium sulfate

c. calcium nitrate

d. iron(III) sulfate

views