Show how Equations 18.7 and 18.9, and the combination reaction that leads to the formation of molecular oxygen, 2O(𝑔)⟶O2(𝑔), can be added to give Equation 18.10.

Verified step by step guidance

1. <b>Step 1:</b> Identify the given equations:</br> - Equation 18.7: This equation likely involves a thermodynamic or kinetic expression related to the formation or dissociation of oxygen species. </br> - Equation 18.9: This equation might describe another aspect of the reaction involving oxygen, such as a different state or energy change.
2. <b>Step 2:</b> Write the combination reaction:</br> The given combination reaction is: \( 2\text{O}(g) \rightarrow \text{O}_2(g) \). This reaction describes the formation of molecular oxygen from atomic oxygen.
3. <b>Step 3:</b> Analyze how the equations can be combined:</br> Consider how the terms in Equations 18.7 and 18.9 relate to the combination reaction. Look for common terms or variables that can be added or subtracted to form a new equation.
4. <b>Step 4:</b> Add the equations:</br> Combine the expressions from Equations 18.7 and 18.9 with the combination reaction. Ensure that the stoichiometry and any thermodynamic or kinetic terms are consistent across the equations.
5. <b>Step 5:</b> Verify the result:</br> Check that the resulting equation matches Equation 18.10. Ensure that all terms are balanced and that the final expression accurately represents the formation of \( \text{O}_2(g) \) from \( \text{O}(g) \).

Key Concepts

Combination Reactions

A combination reaction, also known as a synthesis reaction, occurs when two or more reactants combine to form a single product. This type of reaction is fundamental in chemistry as it illustrates how elements and compounds can interact to create new substances. For example, the formation of molecular oxygen from atomic oxygen, represented as 2O(g) → O2(g), is a classic example of a combination reaction.

Chemical Equations

Chemical equations are symbolic representations of chemical reactions, showing the reactants on the left and the products on the right. They provide a concise way to convey the quantities and states of substances involved in a reaction. Understanding how to balance these equations is crucial for predicting the outcomes of reactions and for stoichiometric calculations, which are essential in quantitative chemistry.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the relationships between the quantities of reactants and products in a chemical reaction. It allows chemists to calculate how much of each substance is needed or produced in a reaction based on the balanced chemical equation. Mastery of stoichiometry is vital for solving problems related to reaction yields, limiting reactants, and the conservation of mass in chemical processes.