Use The Equation Below To Answer The Following Question.How Many Grams Of Potassium Chloride (KCl) Are Produced If 25 G Of Potassium Chlorate \left( KClO_3\right ] Decompose? 2 K C L O 3 → 2 K C L + 3 O 2 2 KClO_3 \rightarrow 2 KCl + 3 O_2 2 K Cl O 3 → 2 K Cl + 3 O 2 A. 10 G KCl B. 15 G

Mar 8, 2025 by ADMIN 293 views

Balancing Chemical Equations and Stoichiometry: A Guide to Calculating Mass of Potassium Chloride (KCl)

Chemical reactions involve the transformation of one or more substances into new substances. These reactions are often represented by chemical equations, which provide a concise representation of the reactants, products, and the stoichiometry of the reaction. In this article, we will explore the concept of balancing chemical equations and stoichiometry, and apply these principles to calculate the mass of potassium chloride (KCl) produced when potassium chlorate (KClO3) decomposes.

A chemical equation is a representation of a chemical reaction, with reactants on the left side and products on the right side. The equation is balanced when the number of atoms of each element is the same on both sides of the equation. This is achieved by adding coefficients in front of the formulas of reactants or products.

The given equation is:

$2 KClO_3 \rightarrow 2 KCl + 3 O_2$

In this equation, the number of potassium (K) atoms is balanced, but the number of chlorine (Cl) atoms is not. To balance the chlorine atoms, we need to add a coefficient of 2 in front of KCl.

$2 KClO_3 \rightarrow 2 KCl + 3 O_2$

However, this equation is still not balanced, as the number of oxygen (O) atoms is not the same on both sides. To balance the oxygen atoms, we need to add a coefficient of 3 in front of O2.

$2 KClO_3 \rightarrow 2 KCl + 3 O_2$

Now, the equation is balanced, with 2 potassium atoms, 2 chlorine atoms, and 6 oxygen atoms on both sides.

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the calculation of the amounts of reactants and products required or produced in a reaction.

In this case, we are given 25 g of potassium chlorate (KClO3) and asked to calculate the mass of potassium chloride (KCl) produced. To do this, we need to use the balanced equation and the molar masses of KClO3 and KCl.

The molar masses of KClO3 and KCl are:

KClO3: 122.55 g/mol
KCl: 74.55 g/mol

To calculate the mass of KCl produced, we need to use the balanced equation and the molar masses of KClO3 and KCl.

From the balanced equation, we can see that 2 moles of KClO3 produce 2 moles of KCl. Therefore, the mole ratio of KClO3 to KCl is 1:1.

We are given 25 g of KClO3, which is equivalent to:

25 g / 122.55 g/mol = 0.204 mol

Since the mole ratio of KClO3 to KCl is 1:1, the number of moles of KCl produced is also 0.204 mol.

The mass of KCl produced is:

0.204 mol x 74.55 g/mol = 15.2 g

Therefore, the mass of potassium chloride (KCl) produced when 25 g of potassium chlorate (KClO3) decomposes is approximately 15 g.

In this article, we have explored the concept of balancing chemical equations and stoichiometry, and applied these principles to calculate the mass of potassium chloride (KCl) produced when potassium chlorate (KClO3) decomposes. We have used the balanced equation and the molar masses of KClO3 and KCl to calculate the mass of KCl produced.

The calculation shows that the mass of KCl produced is approximately 15 g, which is option B. This demonstrates the importance of balancing chemical equations and using stoichiometry to calculate the amounts of reactants and products required or produced in a reaction.

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling
Stoichiometry: A Guide to Calculating Mass and Mole Relationships, by John W. Moore

This article has provided a comprehensive guide to balancing chemical equations and stoichiometry, and has applied these principles to calculate the mass of potassium chloride (KCl) produced when potassium chlorate (KClO3) decomposes.

However, there are some limitations to this calculation. For example, the molar masses of KClO3 and KCl are assumed to be constant, which may not be the case in reality. Additionally, the calculation assumes that the reaction is 100% efficient, which may not be the case in reality.

Therefore, it is essential to consider these limitations when using stoichiometry to calculate the amounts of reactants and products required or produced in a reaction.

The final answer is: B. 15 g
Q&A: Balancing Chemical Equations and Stoichiometry

In our previous article, we explored the concept of balancing chemical equations and stoichiometry, and applied these principles to calculate the mass of potassium chloride (KCl) produced when potassium chlorate (KClO3) decomposes. In this article, we will answer some frequently asked questions (FAQs) related to balancing chemical equations and stoichiometry.

A: The purpose of balancing chemical equations is to ensure that the number of atoms of each element is the same on both sides of the equation. This is essential to accurately predict the amounts of reactants and products required or produced in a reaction.

A: To balance a chemical equation, you need to add coefficients in front of the formulas of reactants or products. The coefficients should be such that the number of atoms of each element is the same on both sides of the equation.

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the calculation of the amounts of reactants and products required or produced in a reaction.

A: To calculate the mass of a product using stoichiometry, you need to use the balanced equation and the molar masses of the reactants and products. You can then use the mole ratio of the reactants and products to calculate the mass of the product.

A: Some common mistakes to avoid when balancing chemical equations and using stoichiometry include:

Not balancing the equation correctly
Not using the correct molar masses of the reactants and products
Not considering the limitations of the calculation (e.g. assuming 100% efficiency)
Not checking the units of the answer

A: To check the units of your answer, you need to ensure that the units of the answer match the units of the question. For example, if the question asks for the mass of a product in grams, the answer should also be in grams.

A: Some real-world applications of balancing chemical equations and stoichiometry include:

Calculating the amounts of reactants and products required for a chemical reaction
Predicting the yields of chemical reactions
Designing chemical reactors and processes
Optimizing chemical reactions for maximum efficiency

In this article, we have answered some frequently asked questions (FAQs) related to balancing chemical equations and stoichiometry. We have also discussed some common mistakes to avoid when balancing chemical equations and using stoichiometry, and some real-world applications of these concepts.

By understanding and applying these concepts, you can accurately predict the amounts of reactants and products required or produced in a reaction, and design chemical reactors and processes that are efficient and effective.

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling
Stoichiometry: A Guide to Calculating Mass and Mole Relationships, by John W. Moore

This article has provided a comprehensive guide to balancing chemical equations and stoichiometry, and has answered some frequently asked questions (FAQs) related to these concepts.

Therefore, it is essential to consider these limitations when using stoichiometry to calculate the amounts of reactants and products required or produced in a reaction.

The final answer is: B. 15 g