Problem 71
Question
Write skeleton equations for these reactions. $$a.\operatorname{iron}(\mathrm{s})+\text { fluorine(g) } \rightarrow$$ $$b. sulfur trioxide(g)+\text { water }(1) \rightarrow \text { sulfuric acid }(a q)$$ $$\begin{array}{c}{\text { c. sodium (s) + magnesium iodide }(a q) \rightarrow} \\ {\text { sodium iodide }(a q)+\text { magnesium (s) }}\end{array}$$ $$d. vanadium (s)+\text { oxygen }(g) \rightarrow \text { vanadium }(V) \text { oxide }(s)$$
Step-by-Step Solution
Verified Answer
Write skeleton equations as: (a) Fe(s) + F2(g) → FeFx, (b) SO3(g) + H2O(l) → H2SO4(aq), (c) Na(s) + MgI2(aq) → NaI(aq) + Mg(s), (d) V(s) + O2(g) → V2O5(s).
1Step 1: Understand the Skeleton Equation
A skeleton equation is a chemical equation that shows only the formulas of the reactants and products, without indicating the amounts of each. It represents the unbalanced chemical reaction.
2Step 2: Write the Skeleton Equation for Reaction (a)
Identify the reactants and products: Iron (Fe) and fluorine (_2) react to form iron fluoride. Write the skeleton equation: \[\text{Fe (s)} + \text{F}_2 (g) \rightarrow \text{FeF}_x (s)\]where \(x\) will be determined when balancing the equation.
3Step 3: Write the Skeleton Equation for Reaction (b)
Identify the reactants and products: Sulfur trioxide (SO_3) and water (H_2O) react to form sulfuric acid (H_2SO_4). Write the skeleton equation: \[\text{SO}_3 (g) + \text{H}_2\text{O} (l) \rightarrow \text{H}_2\text{SO}_4 (aq)\]
4Step 4: Write the Skeleton Equation for Reaction (c)
Identify the reactants and products: Sodium (Na) reacts with magnesium iodide (MgI_2) to form sodium iodide (NaI) and magnesium (Mg). Write the skeleton equation: \[\text{Na (s)} + \text{MgI}_2 (aq) \rightarrow \text{NaI} (aq) + \text{Mg (s)}\]
5Step 5: Write the Skeleton Equation for Reaction (d)
Identify the reactants and products: Vanadium (V) reacts with oxygen (O_2) to form vanadium (V) oxide. Write the skeleton equation: \[\text{V (s)} + \text{O}_2 (g) \rightarrow \text{V}_2\text{O}_5 (s)\]
Key Concepts
Unbalanced Chemical ReactionReactants and ProductsIron FluorideSulfuric AcidSodium IodideVanadium(V) Oxide
Unbalanced Chemical Reaction
An unbalanced chemical reaction is one where the number of atoms of each element are not the same on both sides of the equation. It's an initial step in the conversion of the reactants to products. These reactions require balancing to ensure that the law of conservation of mass is satisfied. The starting point for balancing a chemical equation is a skeleton equation, which is an unbalanced equation that depicts the reactants and products using their respective chemical formulas.
A skeleton equation does not include the quantities of molecules or atoms involved. It's more of a guideline that indicates what substances need to be balanced on either side of the reaction. It helps set the stage for determining the correct coefficients needed to express the chemical reaction accurately.
To balance a chemical equation, you typically adjust the coefficients—the numbers in front of the molecules—until the number of each type of atom on the reactants side equals the number on the products side.
A skeleton equation does not include the quantities of molecules or atoms involved. It's more of a guideline that indicates what substances need to be balanced on either side of the reaction. It helps set the stage for determining the correct coefficients needed to express the chemical reaction accurately.
To balance a chemical equation, you typically adjust the coefficients—the numbers in front of the molecules—until the number of each type of atom on the reactants side equals the number on the products side.
Reactants and Products
In a chemical reaction, the substances initially present are known as reactants, while the substances formed as a result of the reaction are called products. Understanding the distinction between these two is crucial for writing and balancing any chemical equation.
Reactants are the starting materials in any chemical process. They undergo a reaction, facilitated by various conditions like temperature or pressure, to form new substances. For example, in a reaction involving iron and fluorine, iron and fluorine are the reactants, and a compound of iron fluoride is the product.
Reactants are the starting materials in any chemical process. They undergo a reaction, facilitated by various conditions like temperature or pressure, to form new substances. For example, in a reaction involving iron and fluorine, iron and fluorine are the reactants, and a compound of iron fluoride is the product.
- Reactants: Substances that start the reaction.
- Products: New substances formed from the reaction.
Iron Fluoride
Iron fluoride is a general term for compounds composed of iron (Fe) and fluorine (F). These compounds can include different forms, such as iron(II) fluoride (FeF₂) and iron(III) fluoride (FeF₃), depending on the oxidation state of iron.
During a chemical reaction involving iron and fluorine, they combine to form iron fluoride, which is characterized by its ionic nature. This combination is facilitated when iron, a transition metal, reacts with diatomic fluorine gas, a halogen, leading to an electron transfer and formation of a compound like FeF₃.
Writing the skeleton equation helps identify this compound as one of the products of the reaction: - Reactants: Fe and F₂ - Product: FeFₓ, where "x" is determined when balancing the equation.
During a chemical reaction involving iron and fluorine, they combine to form iron fluoride, which is characterized by its ionic nature. This combination is facilitated when iron, a transition metal, reacts with diatomic fluorine gas, a halogen, leading to an electron transfer and formation of a compound like FeF₃.
Writing the skeleton equation helps identify this compound as one of the products of the reaction: - Reactants: Fe and F₂ - Product: FeFₓ, where "x" is determined when balancing the equation.
Sulfuric Acid
Sulfuric acid, with the chemical formula H₂SO₄, is a strong mineral acid widely used in industry and laboratory settings. It forms from the reaction between sulfur trioxide (SO₃) and water (H₂O), which is commonly depicted in chemical equations.
The formation of sulfuric acid is an example of a combination reaction, where simple reactants create a more complex product. The skeleton equation for this process is: - SO₃ (g) + H₂O (l) → H₂SO₄ (aq)
This equation shows the transformation of sulfur trioxide gas and liquid water into sulfuric acid in an aqueous solution, clearly outlining the reactants and the singular product formed through their interaction.
The formation of sulfuric acid is an example of a combination reaction, where simple reactants create a more complex product. The skeleton equation for this process is: - SO₃ (g) + H₂O (l) → H₂SO₄ (aq)
This equation shows the transformation of sulfur trioxide gas and liquid water into sulfuric acid in an aqueous solution, clearly outlining the reactants and the singular product formed through their interaction.
Sodium Iodide
Sodium iodide (NaI) is a stable ionic compound formed from sodium (Na) and iodine. It often results from a chemical reaction in which sodium, a highly reactive metal, combines with iodine, a halogen.
One example is the reaction of sodium with magnesium iodide (MgI₂), resulting in the formation of sodium iodide and solid magnesium. The skeleton equation for this transformation is as follows: - Reactants: Na (s) + MgI₂ (aq) - Products: NaI (aq) + Mg (s)
This skeleton equation highlights the exchange of partners, typical of a replacement reaction where sodium displaces magnesium from magnesium iodide to form sodium iodide.
One example is the reaction of sodium with magnesium iodide (MgI₂), resulting in the formation of sodium iodide and solid magnesium. The skeleton equation for this transformation is as follows: - Reactants: Na (s) + MgI₂ (aq) - Products: NaI (aq) + Mg (s)
This skeleton equation highlights the exchange of partners, typical of a replacement reaction where sodium displaces magnesium from magnesium iodide to form sodium iodide.
Vanadium(V) Oxide
Vanadium(V) oxide (V₂O₅) is an inorganic compound formed by the reaction of vanadium with oxygen. This compound is notable in catalysis and industrial processes, including the production of sulfuric acid.
When solid vanadium reacts with oxygen gas, it forms vanadium(V) oxide. This is depicted in the skeleton equation as: - Reactants: V (s) + O₂ (g) - Product: V₂O₅ (s)
As with other skeleton equations, the exact quantity of each molecule is adjusted during the balancing process. For vanadium(V) oxide, the combination involves multiple atoms of both reactants to produce a stable compound, demonstrating the stoichiometric relationships necessary for balance.
When solid vanadium reacts with oxygen gas, it forms vanadium(V) oxide. This is depicted in the skeleton equation as: - Reactants: V (s) + O₂ (g) - Product: V₂O₅ (s)
As with other skeleton equations, the exact quantity of each molecule is adjusted during the balancing process. For vanadium(V) oxide, the combination involves multiple atoms of both reactants to produce a stable compound, demonstrating the stoichiometric relationships necessary for balance.
Other exercises in this chapter
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