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Chapter 5: Problem 8

Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) reacts with iron metal to make iron(III) sulfate and hydrogen gas. Write a balanced chemical equation that summarizes this reaction.

Short Answer

Expert verified
Balanced equation: \(2\mathrm{Fe} + 3\mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + 3\mathrm{H}_2\).

Step by step solution

01

Write the Unbalanced Chemical Equation

To start, we write the unbalanced chemical equation based on the given substances. Iron metal (\(\mathrm{Fe}\)) reacts with sulfuric acid (\(\mathrm{H}_2\mathrm{SO}_4\)) to produce iron(III) sulfate (\(\mathrm{Fe}_2\mathrm{(SO_4)_3}\)) and hydrogen gas (\(\mathrm{H}_2\)). The unbalanced equation is:\[\mathrm{Fe} + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + \mathrm{H}_2\]
02

Balance the Iron Atoms

Next, we need to balance the number of iron (Fe) atoms on both sides. We see there are two iron atoms in iron(III) sulfate on the product side, so we need two iron atoms on the reactant side:\[\underline{2}\mathrm{Fe} + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + \mathrm{H}_2\]
03

Balance the Sulfate Ions

Then, we balance the sulfate (SO4) ions. Iron(III) sulfate has 3 sulfate ions, so we need 3 sulfuric acid molecules to provide these ions:\[2\mathrm{Fe} + \underline{3}\mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + \mathrm{H}_2\]
04

Balance the Hydrogen Atoms

Now balance the hydrogen (H) atoms. There are 6 hydrogen atoms in 3 \(\mathrm{H}_2\mathrm{SO}_4\). Thus, we need 3 hydrogen molecules (\(\mathrm{H}_2\)) on the product side:\[2\mathrm{Fe} + 3\mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + \underline{3}\mathrm{H}_2\]
05

Verify the Balancing

Finally, verify the equation by counting all atoms of each element on both sides. There are 2 Fe, 3 SO4, and 6 H atoms on both sides, confirming that the equation is balanced:\[2\mathrm{Fe} + 3\mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{Fe}_2\mathrm{(SO_4)_3} + 3\mathrm{H}_2\]

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Key Concepts

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

Sulfuric Acid in the Reaction
Sulfuric acid, chemically represented as \( \text{H}_2\text{SO}_4 \), plays a vital role in this chemical reaction. It is a strong mineral acid composed of two hydrogen atoms, one sulfur atom, and four oxygen atoms.Understanding sulfuric acid is essential because it acts as the reactant in the equation. When sulfuric acid reacts with iron, it helps to form iron(III) sulfate as well as release hydrogen gas. The strength of sulfuric acid enables it to react with metals like iron to produce a sulfate compound. It's important to note that sulfuric acid is both highly corrosive and reacts vigorously with other substances due to its acidic nature. This characteristic makes it a powerful agent in many chemical reactions, including the one described here.
Formation of Iron(III) Sulfate
Iron(III) sulfate, or \( \text{Fe}_2(\text{SO}_4)_3 \), is another key product of this reaction. It forms when iron metal reacts with sulfuric acid. In this context, iron acts as a reducing agent that loses electrons, while the solution of sulfuric acid supplies sulfate ions. The balanced equation indicates that two iron atoms are needed to react with three sulfate ions. In the process, each iron atom becomes oxidized and bonds with sulfate ions to ultimately form iron(III) sulfate. This compound has various applications, particularly in water treatment and as a coagulant in industry. Understanding how it forms in chemical equations is useful for predicting products and knowing the stoichiometry of reactions.
Release of Hydrogen Gas
In the described reaction, hydrogen gas, represented as \( \text{H}_2 \), is released as a byproduct. Hydrogen gas is made up of diatomic molecules where two hydrogen atoms share a pair of electrons.In chemical reaction terms, hydrogen gas is often formed when acids react with metals, which is the case here. When iron and sulfuric acid react, they not only produce iron(III) sulfate but also release hydrogen gas. Hydrogen gas is colorless, odorless, and often used as a fuel source. Its production in metal-acid reactions is essential, both in laboratory settings for various experiments and industrial processes where hydrogen might be implemented in different chemical operations.

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Most popular questions from this chapter

Sulfuric acid is made in a three-step process: (1) the combustion of elemental sulfur to produce sulfur dioxide, (2) the continued reaction of sulfur dioxide with oxygen to produce sulfur trioxide, and (3) the reaction of sulfur trioxide with water to make sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\). Write balanced chemical equations for all three reactions.

Identify each type of reaction. a. \(2 \mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{~s}) \rightarrow 2 \mathrm{~N}_{2}(\mathrm{~g})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})\) b. \(\mathrm{Hg}(\ell)+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{HgO}(\mathrm{s})\) c. \(\mathrm{CH}_{2} \mathrm{CH}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\ell) \rightarrow \mathrm{CH}_{2} \mathrm{BrCH}_{2} \mathrm{Br}\)

Which reactions are redox reactions? For those that are redox reactions, identify the oxidizing and reducing agents. a. \(3 \mathrm{Cu}+8 \mathrm{HNO}_{3} \rightarrow 3 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}+2 \mathrm{NO}+4 \mathrm{H}_{2} \mathrm{O}\) b. \(2 \mathrm{C}_{2} \mathrm{H}_{6}+7 \mathrm{O}_{2} \rightarrow 4 \mathrm{CO}_{2}+6 \mathrm{H}_{2} \mathrm{O}\) c. \(2 \mathrm{NaHCO}_{3} \rightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) d. \(2 \mathrm{~K}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{KOH}+\mathrm{H}_{2}\)

Balance each equation. a. \(\mathrm{NaOH}+\mathrm{H}_{3} \mathrm{PO}_{4} \rightarrow \mathrm{Na}_{3} \mathrm{PO}_{4}+\mathrm{H}_{2} \mathrm{O}\) b. \(\mathrm{N}_{2} \mathrm{H}_{4}+\mathrm{Cl}_{2} \rightarrow \mathrm{N}_{2}+\mathrm{HCl}\) c. \(\mathrm{Na}_{2} \mathrm{~S}+\mathrm{H}_{2} \mathrm{~S} \rightarrow \mathrm{NaSH}\)

a. What is the law of conservation of matter? b. How does the law of conservation of matter apply to chemistry?
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