Question

Silver oxide may be decomposed by strong heating into silver metal and oxygen gas. Write the unbalanced chemical equation for this process.

Short answer

The unbalanced chemical equation for the decomposition of silver oxide (Ag2O) into silver metal (Ag) and oxygen gas (O2) is: \(Ag2O \rightarrow Ag + O2\)

Step-by-step solution

Identify the reactants and products

In this decomposition reaction, silver oxide (Ag2O) is the reactant, and silver metal (Ag) and oxygen gas (O2) are the products.

Write the unbalanced chemical equation

The unbalanced chemical equation can be written using the chemical formulas of the reactants and products: \(Ag2O \rightarrow Ag + O2\)

Key concepts

Chemical Equations

Understanding chemical equations is vital for anyone studying chemistry. It's how we represent chemical reactions on paper. An equation illustrates how reactants transform into products through a chemical process. For instance, decomposing silver oxide into silver and oxygen can be depicted with a chemical equation. The general form of a chemical equation is as follows: Reactants \rightarrow Products. In our example with silver oxide, we begin with the reactant, which is silver oxide (\(Ag2O\)). When heated strongly, it breaks down, or decomposes, into the products: silver metal (\(Ag\)) and oxygen gas (\(O2\)). This process is crucial not only for understanding the reaction at hand but also for predicting the outcome of similar reactions. Chemical equations provide a quick and efficient method to convey a lot of information about chemical processes, making them indispensable tools in the world of science.

To make the chemical equations meaningful and universally understood, they are written using chemical symbols and formulas. This requires familiarity with the periodic table and an understanding of how compounds are formed. Once you've mastered this symbolic language, you can read and write chemical equations, unlocking the rich narrative of chemical transformations.

Reactants and Products

In every chemical equation, there are two key players: the reactants and the products. They are the 'before' and 'after' of the chemical reaction. The reactants are substances that start the reaction, and products are what you get when the reaction is complete. For instance, in the decomposition of silver oxide, there's one reactant and two products. The lone reactant is \(Ag2O\), silver oxide. Upon decomposing, it forms silver metal (\(Ag\)) as one product and oxygen gas (\(O2\)) as the other product. This concept of reactants and products underpins all chemical reactions and will help you understand the conservation of matter. Matter is not created or destroyed but changes forms. So for our reaction, the amount of silver and oxygen that we get as products must have been present in the original silver oxide reactant. Recognizing reactants and products is a foundational skill in chemistry that plays a critical role in understanding how substances interact and change.

Balancing Chemical Equations

When writing chemical equations, it is important to ensure they are balanced. This means there must be the same number of each type of atom on both sides of the equation because according to the law of conservation of mass, atoms cannot be created or destroyed in a chemical reaction. For the given decomposition reaction \(Ag2O \rightarrow Ag + O2\), we have two silver atoms on the reactant side but only one on the product side, and there's half as much oxygen on the product side as needed to balance the oxygen atoms in silver oxide. To balance it, you'd put a coefficient of 2 in front of \(Ag\), to account for the two silver atoms we need. Then, to balance the oxygen, you'd note that we need two atoms of oxygen on the product side as well, which is already present in one molecule of \(O2\). The correctly balanced equation would then look like this: \(2Ag2O \rightarrow 4Ag + O2\). Learning to balance equations is a key part of chemistry that ensures we accurately represent the conservation of mass in chemical reactions. It involves a systematic approach to ensure that every element is accounted for, similar to solving a puzzle with atomic pieces.