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Chapter 15: Problem 29

Write the chemical equation for the reaction between magnesaum metal and hot water.

Short Answer

Expert verified
The balanced chemical equation for the reaction between magnesium metal and hot water is: Mg + 2H2O -> Mg(OH)2 + H2.

Step by step solution

01

Identify the Reactants

The reactants of the reaction are magnesium metal, which is represented as Mg, and hot water, which can be denoted by H2O in its liquid form.
02

Write the Reaction Skeleton

Write down the reactants on the left-hand side of the equation and the expected products on the right-hand side. Magnesium reacting with hot water will typically produce magnesium hydroxide and hydrogen gas. The skeleton of the reaction is: Mg + H2O -> Mg(OH)2 + H2.
03

Balance the Chemical Equation

Ensure that the number of atoms of each element is equal on both sides of the equation. For this reaction, the initial skeleton is already balanced with one atom of magnesium, two atoms of hydrogen and two of oxygen on both sides.

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Key Concepts

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

Chemical Reaction
A chemical reaction is a process in which substances, known as reactants, transform into entirely new substances referred to as products. During this transformation, the atoms of the reactants are rearranged through breaking and forming chemical bonds to create products with different properties.

For instance, when magnesium metal reacts with hot water, a chemical reaction occurs. The magnesium atoms interact with the water molecules (H2O), resulting in the formation of magnesium hydroxide (Mg(OH)2) and hydrogen gas (H2). This change signifies a chemical reaction because it involves a chemical transformation leading to new substances being produced.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the substances involved in a chemical reaction. It is based on the conservation of mass and the concept of the mole, which is a unit used to measure the amount of substance.

To perform stoichiometric calculations, one must understand the mole ratio derived from the coefficients of each substance in a balanced chemical equation. For example, in a balanced equation of magnesium reacting with water, stoichiometry would allow one to calculate how many moles of hydrogen gas are produced from a certain amount of magnesium metal or how much magnesium is required to react with a given amount of water.
Reactants and Products
In any chemical reaction, the reactants are the starting substances present before the reaction occurs, while the products are the substances formed as a result of the reaction.

In the reaction between magnesium and hot water, magnesium (Mg) and water (H2O) are the reactants, and magnesium hydroxide (Mg(OH)2) along with hydrogen gas (H2) are the products. Balancing the reaction equation is crucial as it ensures that the amount of reactants and products is consistent with the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. For teaching purposes, this balance helps students appreciate the need to account for every atom involved in the reaction and serves as the foundation for more advanced concepts in chemistry, such as reaction yield and theoretical versus actual yield analysis.

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Most popular questions from this chapter

The azide ion has an ionic radess of \(148 \mathrm{pm}\) and forms many ionic and covalent compounds that are similar to those of the halides. (a) Write the Lewis formula for the azide ion and predict the \(\mathrm{N}-\mathrm{N}-\mathrm{N}\) bond angle. (b) On the basis of its ionic radius, where in Ciroup 17/VII would you place the azide ion? (c) Compare the acidity of hydrazoic acid with those of the hydrohalic acids and explain any differences (for \(\mathrm{HN}_{3}, K_{2}=1.7 \times\) \(\left.10^{-5}\right\rangle\). (d) Write the formulas of three jonic or coralent azides.

Identify the products and write a balanced equation for the reaction of hydrogen with (a) nitrogen; (b) fluorine; (c) cesium; (d) copper(II) ions.

The nitrosyl ion, \(\mathrm{NO}^{+}\), is isoelectronic with \(\mathrm{N}_{2}\) and has two fewer electrons than \(\mathrm{O}_{2}\). The ion is stable and can be purchased as its hexafloorophosphate \(\left(\mathrm{PF}_{6}{ }^{-}\right)\)or tetrafluoroborate \(\left(\mathrm{BF}_{4}{ }^{-}\right.\)) salt. (a) Draw its molecular orbital diagram and compare it with those of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\). (b) \(\mathrm{NO}^{+}\)is diamagnetic. Can we tell which orbital, the \(\sigma_{2_{p}}\) or the \(\pi_{2_{p}}\), is higher in energy from this information?

Arrange the following atoms in order of increasing first ionization energy: axygen, tellurium, selenium.

Write the chemical equation for the reaction between (a) cesium and oxygen (cesium reacts with oxygen in the same way as potassium); (b) sodium axide and water; (c) lithium and hydrochloric acid; (d) cesium and iodine.
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