Answer:
When referring to fixed ratios that can be expressed as small whole numbers, we are talking about the concept of stoichiometry in chemistry. 1. Fixed ratios: In chemical reactions, substances combine or react with each other in fixed ratios. This means that the number of atoms or molecules involved in a reaction is determined by the stoichiometry of the reaction. These ratios remain constant regardless of the amount of substance used.
Step-by-step explanation:
2. Ratios of small whole numbers: The stoichiometric ratios in a chemical reaction are often expressed as ratios of small whole numbers. This is because chemical reactions involve the rearrangement of atoms or molecules, and these rearrangements occur in simple and predictable ways. 3. Example: Let's consider the reaction between hydrogen (H2) and oxygen (O2) to form water (H2O). The balanced equation for this reaction is: 2H2 + O2 → 2H2O In this reaction, two molecules of hydrogen (H2) react with one molecule of oxygen (O2) to produce two molecules of water (H2O). The stoichiometric ratio between hydrogen and oxygen is 2:1, which can be expressed as a ratio of small whole numbers. Similarly, in many other chemical reactions, the stoichiometric ratios can be expressed as simple fractions or ratios of small whole numbers. This is because atoms combine in specific ways to form compounds, and these combinations follow predictable patterns. In summary, fixed ratios in chemistry refer to the stoichiometry of chemical reactions. These ratios can be expressed as ratios of small whole numbers, representing the number of atoms or molecules involved in the reaction. An example is the stoichiometric ratio of 2:1 between hydrogen and oxygen in the reaction that forms water.