Write balanced equations for the reactions between each of the following oxides and water: (a) \(\mathrm{Li}_{2} \mathrm{O}\) (b) \(\mathrm{CaO},\) (c) \(\mathrm{SO}_{3}\).

Short Answer

Expert verified
The balanced equations for the reactions are:(a) \(\mathrm{Li}_{2} \mathrm{O}_{(s)} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow 2 \mathrm{LiOH}_{(aq)}\)(b) \(\mathrm{CaO}_{(s)} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{Ca(OH)}_{2 _{(s)}}\)(c) \(\mathrm{SO}_{3 _{(g)}} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4 _{(aq)}}\)

Step by step solution

01

Reacting Lithium Oxide with Water

Here, lithium oxide (Li2O) reacts with water (H2O) to form lithium hydroxide, which is a base. The balanced equation is: \[\mathrm{Li}_{2} \mathrm{O}_{(s)} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow 2 \mathrm{LiOH}_{(aq)}\] This indicates that one mole of lithium oxide reacts with one mole of water to produce two moles of lithium hydroxide.
02

Reacting Calcium Oxide with Water

Calcium oxide (CaO) reacts with water (H2O) to form calcium hydroxide, another base. The balanced equation for this reaction is: \[\mathrm{CaO}_{(s)} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{Ca(OH)}_{2 _{(s)}}\]Here, one mole of calcium oxide reacts with one mole of water to produce one mole of calcium hydroxide.
03

Reacting Sulfur Trioxide with Water

Sulfur trioxide (SO3) reacts with water (H2O) to form sulfuric acid, which is an acid. The balanced equation for this reaction is: \[\mathrm{SO}_{3 _{(g)}} + \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4 _{(aq)}}\]This indicates that one mole of sulfur trioxide reacts with one mole of water to produce one mole of sulfuric acid.

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Key Concepts

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

Reaction of Oxides with Water
Understanding the reaction of oxides with water is essential for grasping the basics of inorganic chemistry. Oxides are compounds that contain one or more oxygen atoms bound to another element. When they react with water, they often form new substances such as bases or acids depending on the nature of the oxide.

For example, metal oxides tend to undergo a synthesis reaction with water to produce metal hydroxides. In contrast, nonmetal oxides typically react to form acids. These reactions are fundamental in environmental chemistry. For instance, carbon dioxide dissolves in rainwater to form carbonic acid, affecting the pH of natural water systems.
Forming Bases from Metal Oxides
Metal oxides are known for reacting with water to form bases. A base is a substance that can accept protons (hydrogen ions) or donate a pair of valence electrons to form a bond. They have a pH greater than 7 and are characterized by their ability to neutralize acids.

In the given exercise, we see this phenomenon with lithium oxide (Li2O) and calcium oxide (CaO). When they come in contact with water (H2O), they form lithium hydroxide (LiOH) and calcium hydroxide (Ca(OH)2) respectively. These reactions can be categorized as a type of hydrolysis where the metal oxide acts as the base-forming agent in the presence of water.
Forming Acids from Nonmetal Oxides
In contrast to metal oxides, nonmetal oxides react with water to form acidic solutions. Acids are substances that donate hydrogen ions (H+) when dissolved in water and have a pH less than 7. They are known for their sour taste and ability to corrode metals.

Take sulfur trioxide (SO3) for instance. When it comes into contact with water, it forms sulfuric acid (H2SO4), one of the most important industrial acids used in battery acid and various cleaning agents. This process of forming acids from nonmetal oxides is crucial in understanding acid rain and environmental effects caused by industrial emissions that increase acidity in natural waters.
Chemical Equation Balancing
Chemical equation balancing is at the heart of chemical reactions. To satisfy the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction, the number of atoms for each element must be the same on both sides of the equation. This ensures that the reaction adheres to the principle of mass balance.

To balance a chemical equation, like those presented in the exercise with Li2O, CaO, and SO3, one must adjust the coefficients - the numbers placed before compounds - to get the same number of atoms of each element on both sides of the equation. It's a bit like a puzzle, where you need to make sure that every atom that goes into the reaction comes out, whether as a reactant or as a part of the products.

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Most popular questions from this chapter

Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

Sketch the outline of the periodic table and show group and period trends in the first ionization energy of the elements. What types of elements have the highest ionization energies and what types the lowest ionization energies?

Arsenic (As) is not an essential element for the human body. (a) Based on its position in the periodic table, suggest a reason for its toxicity. (b) When arsenic enters a person's body, it quickly shows up in the follicle of the growing hair. This action has enabled detectives to solve many murder mysteries by analyzing a victim's hair. Where else might one look for the accumulation of the element if arsenic poisoning is suspected?

One allotropic form of an element \(X\) is a colorless crystalline solid. The reaction of \(\mathrm{X}\) with an excess amount of oxygen produces a colorless gas. This gas dissolves in water to yield an acidic solution. Choose one of the following elements that matches \(\mathrm{X}:\) (a) sulfur, (b) phosphorus, (c) carbon, (d) boron, and (e) silicon.

A technique called photoelectron spectroscopy is used to measure the ionization energy of atoms. A sample is irradiated with UV light, and electrons are ejected from the valence shell. The kinetic energies of the ejected electrons are measured. Because the energy of the UV photon and the kinetic energy of the ejected electron are known, we can write $$ h \nu=I E+\frac{1}{2} m u^{2} $$ where \(\nu\) is the frequency of the UV light, and \(m\) and \(u\) are the mass and velocity of the electron, respectively. In one experiment the kinetic energy of the ejected electron from potassium is found to be \(5.34 \times 10^{-19} \mathrm{~J}\) using a UV source of wavelength \(162 \mathrm{nm} .\) Calculate the ionization energy of potassium. How can you be sure that this ionization energy corresponds to the electron in the valence shell (that is, the most loosely held electron)?

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