Question

Oxygen can be produced by the decomposition of potassium chlorate, \(\mathrm{KClO}_{3}\). The products of the reaction are \(\mathrm{KCl}\) and \(\mathrm{O}_{2}\). Write a balanced equation for the reaction.

Short answer

The balanced equation for the decomposition of potassium chlorate into potassium chloride and oxygen is \(2\mathrm{KClO}_{3} \rightarrow 2\mathrm{KCl} + 3\mathrm{O}_{2}\).

Step-by-step solution

Write the unbalanced equation

First, let's write down the unbalanced chemical equation using the chemical formula of the reactants and products: \(\mathrm{KClO}_{3} \rightarrow \mathrm{KCl} + \mathrm{O}_{2}\)

Balance the equation

Now, we will balance the equation by adjusting the coefficients (the numbers in front of the chemical formulas) of the reactants and products. 1. Count the number of atoms for each element on both sides of the equation: Reactant side: - 1 K atom - 1 Cl atom - 3 O atoms Product side: - 1 K atom - 1 Cl atom - 2 O atoms (in one O₂ molecule) 2. Notice that the number of oxygen atoms is not balanced. To balance the oxygen atoms, place a coefficient of 2 in front of the potassium chlorate molecule: \(2\mathrm{KClO}_{3} \rightarrow \mathrm{KCl} + \mathrm{O}_{2}\) Now, we have: Reactant side: - 2 K atoms - 2 Cl atoms - 6 O atoms 3. To balance the K and Cl atoms, place a coefficient of 2 in front of the potassium chloride molecule: \(2\mathrm{KClO}_{3} \rightarrow 2\mathrm{KCl} + \mathrm{O}_{2}\) Now, we have: Product side: - 2 K atoms - 2 Cl atoms - 2 O atoms (in one O₂ molecule) * 2 = 4 O atoms 4. Finally, place a coefficient of 3 in front of the oxygen molecule to balance the oxygen atoms: \(2\mathrm{KClO}_{3} \rightarrow 2\mathrm{KCl} + 3\mathrm{O}_{2}\) Now, we have: Product side: - 2 K atoms - 2 Cl atoms - 2 O atoms (in one O₂ molecule) * 3 = 6 O atoms The equation is now balanced, and the final balanced chemical equation is: \(2\mathrm{KClO}_{3} \rightarrow 2\mathrm{KCl} + 3\mathrm{O}_{2}\)

Key concepts

Oxygen Production

Oxygen is a vital component for all forms of life. Producing oxygen through chemical reactions is an essential area of research and practice in chemistry. One common method involves the decomposition of compounds that contain oxygen, such as potassium chlorate (\(\mathrm{KClO}_3\)).

• Oxygen is released as one of the products in the decomposition of potassium chlorate.
• The reaction not only highlights the production of oxygen but also serves as a classic example of generating gases from solids in a laboratory setting.

Understanding this method can help students and chemists develop other ways to safely produce oxygen for different applications. For instance, fireworks industries use this reaction for oxygen production to intensify the burn, making the fireworks dazzle in the sky. With a well-balanced chemical equation, oxygen generation can be controlled effectively to meet the desired experimental conditions.

Chemical Decomposition

Chemical decomposition is a type of chemical reaction where a single compound breaks down into two or more simpler substances. It is the opposite of combination reactions, where substances combine to form a new compound. In the decomposition of potassium chlorate (\(\mathrm{KClO}_3\)), it breaks down into potassium chloride (\(\mathrm{KCl}\)) and oxygen gas (\(\mathrm{O}_2\)).

• This reaction is significant because it demonstrates how a more complex compound can be broken down into simpler components.
• Decomposition requires energy, often in the form of heat, to overcome the forces holding the compound together.

This process can be observed in various fields such as pharmaceutical manufacturing, where similar reactions are used to obtain raw materials from complex compounds. Chemists manipulate conditions, like temperature, to favor decomposition and obtain desired products.

Chemical Reaction

A chemical reaction involves the transformation of reactants into products. When potassium chlorate decompose, a chemical reaction takes place converting it into potassium chloride and oxygen gas. This type of reaction is fundamental in chemistry as it establishes an understanding of how substances interact.

• During a chemical reaction, bonds between atoms are broken and reformed, leading to new substances being produced.
• Not all systems require visible changes; some reactions, like color changes or gas production, are more detectable.

In the case of potassium chlorate decomposition, the reaction is visible through the evolution of gas bubbles or even a slight rise in gas temperature. This knowledge is applied in many practical applications, including forensic science and environmental monitoring, where understanding these transformations help in assessing chemical compositions and outcomes.

Stoichiometry

Stoichiometry is a branch of chemistry dealing with quantitative relationships in chemical reactions. It involves using balanced chemical equations to calculate the amounts of reactants and products involved in a reaction.In the decomposition reaction of potassium chlorate, stoichiometry helps us determine:

• The coefficients needed to balance the equation ensuring mass conservation.
• This tells us, precisely, how much product we can expect from a given amount of reactant.

For the balanced equation (\(2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl} + 3 \mathrm{O}_{2}\)), stoichiometry can tell us how many moles of oxygen are produced for moles of potassium chlorate decomposed. Such calculations are crucial for industrial applications, where optimal handling of raw materials is essential for economic and sustainability considerations.