Review The Equation Below.$\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \\]How Many Moles Of Oxygen Are Produced When 2 Mol Of Potassium Chlorate \[$(\text{KClO}_3)\$\] Decompose?A. 1 B. 2 C. 3 D. 6

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Balancing Chemical Equations and Stoichiometry: A Review of the Decomposition of Potassium Chlorate

Chemical equations are a fundamental concept in chemistry, allowing us to describe the reactants and products involved in a chemical reaction. However, not all chemical equations are balanced, meaning that the number of atoms of each element is the same on both the reactant and product sides. In this article, we will review the equation for the decomposition of potassium chlorate (KClO3) and use it to determine the number of moles of oxygen produced when 2 mol of potassium chlorate decompose.

The Balanced Equation

The given equation for the decomposition of potassium chlorate is:

2KClO3→2KCl+3O2{ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 }

This equation is already balanced, meaning that the number of atoms of each element is the same on both the reactant and product sides. The balanced equation indicates that 2 mol of potassium chlorate decompose to produce 2 mol of potassium chloride (KCl) and 3 mol of oxygen (O2).

Stoichiometry and Mole Ratios

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. In this case, we are interested in determining the number of moles of oxygen produced when 2 mol of potassium chlorate decompose. To do this, we need to use the mole ratio between potassium chlorate and oxygen from the balanced equation.

The mole ratio between potassium chlorate and oxygen is 2:3, meaning that for every 2 mol of potassium chlorate, 3 mol of oxygen are produced. Since we are given 2 mol of potassium chlorate, we can use this mole ratio to determine the number of moles of oxygen produced.

Calculating the Number of Moles of Oxygen

To calculate the number of moles of oxygen produced, we can use the mole ratio between potassium chlorate and oxygen. Since the mole ratio is 2:3, we can set up a proportion to determine the number of moles of oxygen produced:

2 mol KClO33 mol O2=2 mol KClO3x mol O2{ \frac{2 \text{ mol KClO}_3}{3 \text{ mol O}_2} = \frac{2 \text{ mol KClO}_3}{x \text{ mol O}_2} }

Solving for x, we get:

x=3 mol O22 mol KClO3×2 mol KClO3{ x = \frac{3 \text{ mol O}_2}{2 \text{ mol KClO}_3} \times 2 \text{ mol KClO}_3 }

x=3 mol O2{ x = 3 \text{ mol O}_2 }

Therefore, when 2 mol of potassium chlorate decompose, 3 mol of oxygen are produced.

In conclusion, the balanced equation for the decomposition of potassium chlorate is:

2KClO3→2KCl+3O2{ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 }

Using the mole ratio between potassium chlorate and oxygen, we can determine that 3 mol of oxygen are produced when 2 mol of potassium chlorate decompose. This is a classic example of stoichiometry in action, where the quantitative relationships between reactants and products are used to determine the number of moles of a product produced.

  • The balanced equation for the decomposition of potassium chlorate is: 2KClO3→2KCl+3O2{ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 }
  • The mole ratio between potassium chlorate and oxygen is 2:3.
  • When 2 mol of potassium chlorate decompose, 3 mol of oxygen are produced.
  • What is the balanced equation for the decomposition of potassium chlorate? The balanced equation for the decomposition of potassium chlorate is: 2KClO3→2KCl+3O2{ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 }
  • How many moles of oxygen are produced when 2 mol of potassium chlorate decompose? When 2 mol of potassium chlorate decompose, 3 mol of oxygen are produced.
  • What is the mole ratio between potassium chlorate and oxygen? The mole ratio between potassium chlorate and oxygen is 2:3.
    Q&A: Balancing Chemical Equations and Stoichiometry

In our previous article, we reviewed the equation for the decomposition of potassium chlorate (KClO3) and used it to determine the number of moles of oxygen produced when 2 mol of potassium chlorate decompose. In this article, we will continue to explore the topic of balancing chemical equations and stoichiometry by answering some frequently asked questions.

Q: What is the difference between a balanced equation and an unbalanced equation?

A: A balanced equation is an equation in which the number of atoms of each element is the same on both the reactant and product sides. An unbalanced equation, on the other hand, is an equation in which the number of atoms of each element is not the same on both the reactant and product sides.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to make sure that the number of atoms of each element is the same on both the reactant and product sides. You can do this by adding coefficients (numbers in front of the formulas of the reactants or products) to balance the equation.

Q: What is stoichiometry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the mole ratios between reactants and products to determine the amounts of substances that will be produced or consumed in a reaction.

Q: How do I use mole ratios to determine the amounts of substances that will be produced or consumed in a reaction?

A: To use mole ratios to determine the amounts of substances that will be produced or consumed in a reaction, you need to follow these steps:

  1. Write down the balanced equation for the reaction.
  2. Identify the mole ratio between the reactants and products.
  3. Use the mole ratio to set up a proportion.
  4. Solve the proportion to determine the amount of the substance that will be produced or consumed.

Q: What is the mole ratio between potassium chlorate and oxygen in the decomposition reaction?

A: The mole ratio between potassium chlorate and oxygen in the decomposition reaction is 2:3. This means that for every 2 mol of potassium chlorate, 3 mol of oxygen are produced.

Q: How many moles of oxygen are produced when 2 mol of potassium chlorate decompose?

A: When 2 mol of potassium chlorate decompose, 3 mol of oxygen are produced.

Q: What is the importance of balancing chemical equations and using stoichiometry in chemistry?

A: Balancing chemical equations and using stoichiometry are important in chemistry because they allow us to predict the amounts of substances that will be produced or consumed in a reaction. This is crucial in many areas of chemistry, including chemical engineering, materials science, and environmental science.

In conclusion, balancing chemical equations and using stoichiometry are essential skills in chemistry. By understanding how to balance chemical equations and use mole ratios to determine the amounts of substances that will be produced or consumed in a reaction, we can predict the outcomes of chemical reactions and make informed decisions in many areas of chemistry.

  • A balanced equation is an equation in which the number of atoms of each element is the same on both the reactant and product sides.
  • Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction.
  • The mole ratio between potassium chlorate and oxygen in the decomposition reaction is 2:3.
  • When 2 mol of potassium chlorate decompose, 3 mol of oxygen are produced.
  • What is the difference between a balanced equation and an unbalanced equation? A balanced equation is an equation in which the number of atoms of each element is the same on both the reactant and product sides. An unbalanced equation, on the other hand, is an equation in which the number of atoms of each element is not the same on both the reactant and product sides.
  • How do I balance a chemical equation? To balance a chemical equation, you need to make sure that the number of atoms of each element is the same on both the reactant and product sides. You can do this by adding coefficients (numbers in front of the formulas of the reactants or products) to balance the equation.
  • What is stoichiometry? Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the mole ratios between reactants and products to determine the amounts of substances that will be produced or consumed in a reaction.