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Chapter 20: Problem 28

Elemental boron is produced by reduction of boron oxide with magnesium to give boron and magnesium oxide. Write a balanced equation for this reaction.

Short Answer

Expert verified
The balanced equation for the reaction between boron oxide and magnesium to produce elemental boron and magnesium oxide is: \(B_2O_3 + 3Mg \rightarrow 2B + 3MgO\).

Step by step solution

01

Identify reactants and products

The given information states that the reactants are boron oxide (B₂O₃) and magnesium (Mg), and the products are elemental boron (B) and magnesium oxide (MgO). So, the reaction will look like: B₂O₃ + Mg → B + MgO
02

Write the unbalanced equation

Now, we will write the unbalanced equation using the identified reactants and products: B₂O₃ + Mg → B + MgO
03

Balance the equation

To balance the equation, we need to make sure the number of atoms for each element on both sides of the equation is equal. Let's start by balancing the boron (B) atoms: We have 2 boron atoms on the left side and 1 on the right side. We can add a coefficient of 2 to the boron atom on the right side: B₂O₃ + Mg → 2B + MgO Now, we need to balance the oxygen (O) atoms. We have 3 oxygen atoms on the left side and 1 on the right side. We can add a coefficient of 3 to the magnesium oxide (MgO) on the right side: B₂O₃ + Mg → 2B + 3MgO Finally, we need to balance the magnesium (Mg) atoms. We have 1 magnesium atom on the left side and 3 on the right side. We can add a coefficient of 3 to the magnesium atom on the left side: B₂O₃ + 3Mg → 2B + 3MgO Now, the equation is balanced, as there are the same number of boron, oxygen, and magnesium atoms on both sides of the equation. So the balanced equation is: B₂O₃ + 3Mg → 2B + 3MgO

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
Chemical reactions are processes in which substances, known as reactants, transform into new substances called products. These transformations involve the breaking and forming of chemical bonds, leading to changes in the composition and often properties of the involved substances. Reactions can release or absorb energy and occur in various forms such as synthesis, decomposition, single replacement, double replacement, and combustion.

In the context of elemental boron production, the reduction of boron oxide (B₂O₃) by magnesium (Mg) is a specific type of chemical reaction. Here, magnesium serves as a reducing agent that donates electrons to boron oxide, resulting in the formation of elemental boron (B) and magnesium oxide (MgO). During this process, the magnesium is oxidized while the boron is reduced, showcasing a redox reaction.
Stoichiometry
Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It is based on the conservation of mass, which states that mass cannot be created or destroyed in a chemical reaction. Thus, the amount of each substance involved must be accounted for, often using the mole concept as a way to measure quantities of atoms and molecules.

In stoichiometric calculations, balanced chemical equations are essential because they provide the mole ratio of reactants and products necessary to determine the quantities needed or produced. When balancing the equation for the production of elemental boron, it becomes clear that one mole of B₂O₃ reacts with three moles of Mg to produce two moles of B and three moles of MgO. This mole ratio is crucial for predicting the amount of each substance required or formed in a given reaction.
Chemical Equation Balancing
Balancing chemical equations is a fundamental step in understanding chemical reactions. It involves changing the coefficients of reactants and products to ensure that the number of atoms of each element is the same on both sides of the reaction equation, aligning with the law of conservation of mass.

During the balancing process, it is essential to systematically approach one element at a time. For the boron oxide reduction reaction, start by balancing the boron atoms, followed by oxygen, and lastly magnesium. Each step must be checked and adjusted as necessary to maintain balance for all elements. The balanced equation, B₂O₃ + 3Mg → 2B + 3MgO, shows that three magnesium atoms are needed to produce two boron atoms while forming three units of magnesium oxide, thus maintaining the balance of atoms before and after the reaction.
Elemental Boron Production
Elemental boron is a valuable material with high-strength, lightweight properties, and it can be produced by several methods, including the direct reduction of boron oxide with a strong reducing agent like magnesium. The chemical reduction process is typically carried out in high-temperature conditions, where magnesium reduces the boron oxide to free boron while forming magnesium oxide as a byproduct.

This production method's efficiency depends on a precise stoichiometric balance to ensure complete reduction. In industrial processes, optimizing this reaction involves not only balancing the chemical equation but also controlling the reaction conditions such as temperature, pressure, and the purity of reactants to achieve the desired yield of elemental boron.

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