Question

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Ozone decomposes to dioxygen. (b) Xenon reacts with fluorine. (Write three different equations.) (c) Sulfur reacts with hydrogen gas. (d) Fluorine reacts with water.

Short answer

(a) \(2O_3 → 3O_2\) (b) 1. \(Xe + 3F_2 → XeF_6\) 2. \(Xe + 2F_2 → XeF_4\) 3. Xe + F2 → XeF2 (c) \(S + 2H_2 → 2H_2S\) (d) \(F_2 + H_2O → OF_2 + 2HF\)

Step-by-step solution

Identify reactants and products

The given information is that ozone (O3) decomposes into dioxygen (O2). So, ozone is the reactant and dioxygen is the product.

Write the unbalanced equation

The unbalanced equation for the decomposition of ozone is: O3 → O2

Balance the equation

In the unbalanced equation, there are three oxygen atoms on the left and two oxygen atoms on the right. To balance the equation, we should multiply the product side by \(\frac{3}{2}\). However, we cannot have a fraction as a coefficient in a balanced equation, so we will multiply both sides by 2 to establish whole number coefficients. Therefore, the balanced equation is: \[2O_3 → 3O_2\] ### Case (b): Xenon reacts with fluorine (3 different equations) ###

Identify reactants, possible products, and write the unbalanced equations

The given information is that xenon (Xe) reacts with fluorine (F2). So, xenon and fluorine are the reactants. Xenon can form multiple fluorides: XeF2, XeF4, and XeF6. We will write the balanced equation for each case.

Balance the equations

1. For Xenon Hexafluoride (XeF6): Unbalanced equation: Xe + F2 → XeF6 To balance this equation, add a coefficient of 3 to F2: \[Xe + 3F_2 → XeF_6\] 2. For Xenon Tetrafluoride (XeF4) Unbalanced equation: Xe + F2 → XeF4 To balance this equation, add a coefficient of 2 to F2: \[Xe + 2F_2 → XeF_4\] 3. For Xenon Difluoride (XeF2) Unbalanced equation: Xe + F2 → XeF2 This equation is already balanced. ### Case (c): Sulfur reacts with hydrogen gas ###

Identify reactants and products

The given information is that sulfur (S) reacts with hydrogen gas (H2). So, sulfur and hydrogen gas are the reactants, and the product is Hydrogen Sulfide (H2S).

Write the unbalanced equation

The unbalanced equation for the reaction between sulfur and hydrogen gas is: S + H2 → H2S

Balance the equation

To balance the equation, add a coefficient of 2 to H2S: \[S + 2H_2 → 2H_2S\] ### Case (d): Fluorine reacts with water ###

Identify reactants and products

The given information is that fluorine (F2) reacts with water (H2O). So, fluorine and water are the reactants, and the products are Oxygen Difluoride (OF2) and Hydrogen Fluoride (HF).

Write the unbalanced equation

The unbalanced equation for the reaction between fluorine and water is: F2 + H2O → OF2 + HF

Balance the equation

To balance this equation, add a coefficient of 2 to HF: \[F_2 + H_2O → OF_2 + 2HF\]

Key concepts

Balancing Chemical Equations

Balancing chemical equations is crucial in understanding how chemical reactions work. The goal is to have the same number of each type of atom on both sides of the equation. Consider the decomposition of ozone into dioxygen. We start by writing the unbalanced equation: \( O_3 \rightarrow O_2 \).
As seen, there are three oxygen atoms on the left but only two on the right. To handle this, multiply the dioxygen by \( \frac{3}{2} \), effectively making \( O_2 \) have three oxygen atoms. However, coefficients in chemical equations should be whole numbers. Thus, multiply both sides by 2 to get \( 2O_3 \rightarrow 3O_2 \).
This balancing process confirms the mass conservation principle, ensuring that atoms are neither created nor destructed in the reaction.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. It helps determine the proportions needed for reactants to react completely without excess. Let's use xenon's reactions with fluorine as an example. Xenon can create different compounds with fluorine: XeF2, XeF4, and XeF6.
* For XeF6, the balanced reaction is \( Xe + 3F_2 \rightarrow XeF_6 \). Here, 1 mole of xenon reacts with 3 moles of \( F_2 \).
* For XeF4, the reaction is \( Xe + 2F_2 \rightarrow XeF_4 \), with 1 mole of xenon to 2 moles of \( F_2 \).
* Finally, \( XeF_2 \) only needs \( Xe + F_2 \rightarrow XeF_2 \).
These stoichiometric ratios are essential for calculating the amounts of reactants used and products formed, ensuring reactions are efficient and resources are not wasted.

Types of Chemical Reactions

Chemical reactions can be classified into various types like synthesis, decomposition, single replacement, and more. Understanding these helps predict products and understand the chemical behavior. Let's explore the types through the original reactions:
* **Decomposition Reaction**: Ozone decomposing to dioxygen is a decomposition reaction. One compound breaks down into two or more simpler products: \( 2O_3 \rightarrow 3O_2 \).
* **Synthesis Reaction**: When sulfur reacts with hydrogen, it forms hydrogen sulfide. This is a synthesis reaction, combining elements to form a compound: \( S + 2H_2 \rightarrow 2H_2S \).
* **Single Replacement Reaction**: Fluorine reacting with water exemplifies single replacement, where an element in one compound is replaced by another: \( F_2 + H_2O \rightarrow OF_2 + 2HF \).
Recognizing these types clarifies how reactions proceed and what products to expect.