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Chapter 7: Problem 99

Marine Chemistry of Iron On the seafloor, solid iron(II) oxide may react with water to form solid \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) and hydrogen gas. a. Write a balanced chemical equation for the reaction. b. When \(\mathrm{CO}_{2}\) is also present, the product of the reaction is methane, not hydrogen. Write a balanced chemical equation for this reaction.

Short Answer

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Question: Write the balanced chemical equations for the following reactions: 1. The reaction between solid iron(II) oxide and water to form solid Fe3O4 and hydrogen gas. 2. The reaction between solid iron(II) oxide, water, and CO2 to form methane and any other products. Answer: 1. The balanced chemical equation for the reaction between solid iron(II) oxide and water is: \[3\mathrm{FeO \ (s)} + 2\mathrm{H_{2}O \ (l)} \rightarrow \mathrm{Fe_{3}O_{4} \ (s)} + \mathrm{H_{2} \ (g)}\] 2. The balanced chemical equation for the reaction between solid iron(II) oxide, water, and CO2 to form methane is: \[3\mathrm{FeO \ (s)} + 2\mathrm{H_{2}O \ (l)} + 3\mathrm{CO_{2} \ (g)} \rightarrow 2\mathrm{CH_{4} \ (g)} + \mathrm{Fe_{3}O_{4} \ (s)}\]

Step by step solution

01

Write the balanced reaction between iron(II) oxide and water

The unbalanced equation is FeO (s) + H2O (l) -> Fe3O4 (s) + H2 (g) As there are 3 Fe atoms on the right side and only 1 on the left, we need to multiply FeO by 3: 3FeO (s) + H2O (l) -> Fe3O4 (s) + H2 (g) Now, count the oxygen and hydrogen atoms. On the left side, there are 3 O and 2 H, while on the right side, there are 4 O and 2 H. Balance the oxygen with a coefficient of 2 in front of the H2O to have 4 oxygen atoms on each side: 3FeO (s) + 2H2O (l) -> Fe3O4 (s) + H2 (g) The balanced reaction is: \[3\mathrm{FeO \ (s)} + 2\mathrm{H_{2}O \ (l)} \rightarrow \mathrm{Fe_{3}O_{4} \ (s)} + \mathrm{H_{2} \ (g)}\]
02

Write the balanced reaction between iron(II) oxide, water, and CO2 to form methane

The unbalanced equation contains iron(II) oxide (FeO), water (H2O), CO2, and methane (CH4). FeO (s) + H2O (l) + CO2 (g) -> CH4 (g) + ? Since FeO is the source of iron, the possible iron-containing product is Fe3O4, like in the previous reaction. FeO (s) + H2O (l) + CO2 (g) -> CH4 (g) + Fe3O4 (s) Now balance the reaction: 3FeO (s) + 2H2O (l) + 3CO2 (g) -> 2CH4 (g) + Fe3O4 (s) The balanced reaction is: \[3\mathrm{FeO \ (s)} + 2\mathrm{H_{2}O \ (l)} + 3\mathrm{CO_{2} \ (g)} \rightarrow 2\mathrm{CH_{4} \ (g)} + \mathrm{Fe_{3}O_{4} \ (s)}\]

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Key Concepts

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

Iron Oxide Reactions
Iron oxide reactions, especially involving iron(II) oxide ( FeO ), play a significant role in marine chemistry.
When iron(II) oxide comes into contact with water, it undergoes a chemical reaction. This reaction is important on the seafloor. It transitions iron(II) oxide into magnetite ( Fe鈧僌鈧� ) and hydrogen gas ( H鈧� ).
- In this particular reaction, iron(II) oxide ( FeO(s) ) reacts with water ( H鈧侽(l) ). - The products are solid Fe鈧僌鈧� (s) and hydrogen gas ( H鈧�(g) ). Chemists often explore these reactions to understand how minerals transform underwater.
Factors like temperature and pressure also influence how efficiently these reactions occur in marine environments. This knowledge is crucial for geochemists studying the ocean floor and its compositions.
Balanced Chemical Equation
A balanced chemical equation shows the conservation of mass. This means the same number of each type of atom is present on both sides of a chemical equation.
Let's consider the reaction of iron(II) oxide with water:- Begin with writing the unbalanced equation: FeO (s) + H鈧侽 (l) \( \rightarrow \) Fe鈧僌鈧� (s) + H鈧� (g).- Balancing involves adjusting the number of units to equalize each atom type.Here is how we balance this reaction:- **Fe**: There are three iron atoms (Fe) in Fe鈧僌鈧�, meaning you need three FeO units on the left side.- **O**: To balance oxygen, consider the total oxygen atoms in Fe鈧僌鈧� (4) and H鈧侽.- **H**: Place a coefficient of 2 in front of H鈧侽.The resulted balanced equation is:\[3\mathrm{FeO(s)} + 2\mathrm{H_{2}O(l)} \rightarrow \mathrm{Fe_{3}O_{4}(s)} + \mathrm{H_{2}(g)} \]
Methane Formation
Methane formation involves a shift in products when carbon dioxide (CO鈧�) is present with iron(II) oxide and water.
The presence of CO鈧� alters the outcome of the previous reaction significantly.- Instead of producing hydrogen gas, the reaction outputs methane gas (CH鈧�).- Methane is a significant contributor to Earth's gaseous resources and helps in studies related to energy and environmental science.In the presence of water and CO鈧�:- The reactants are iron(II) oxide and carbon dioxide along with water.- After balancing the equation, the correct proportions result in:\[3\mathrm{FeO (s)} + 2\mathrm{H_{2}O (l)} + 3\mathrm{CO_{2} (g)} \rightarrow 2\mathrm{CH_{4} (g)} + \mathrm{Fe_{3}O_{4} (s)} \]This reaction is a fantastic example of the interplay between geological processes and atmospheric chemistry. Understanding such interactions aids in comprehending the broader cycles involving carbon and their environmental impacts. By balancing these equations, you can accurately represent and study real-world chemical reactions.

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Most popular questions from this chapter

Mining for Gold Unlike most metals, gold occurs in nature as the pure element. Miners in California in 1849 searched for gold nuggets and gold dust in streambeds, where the denser gold could be easily separated from sand and gravel. However, larger deposits of gold are found in veins of rock and can be separated chemically in the following two-step process: (1) \(4 \mathrm{Au}(s)+8 \mathrm{NaCN}(a q)+\mathrm{O}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow\) $$4 \mathrm{NaAu}(\mathrm{CN})_{2}(a q)+4 \mathrm{NaOH}(a q)$$ (2) \(2 \mathrm{NaAu}(\mathrm{CN})_{2}(a q)+\mathrm{Zn}(s) \rightarrow\) $$2 \mathrm{Au}(s)+\mathrm{Na}_{2}\left[\mathrm{Zn}(\mathrm{CN})_{4}\right](a q)$$ If 23 kilograms of ore is \(0.19 \%\) gold by mass, how much Zn is needed to react with the gold in the ore? Assume that reactions 1 and 2 are \(100 \%\) efficient.

Corn farmers in the American Midwest typically use \(5.0 \times 10^{3}\) kilograms of ammonium nitrate fertilizer per square kilometer of cornfield per year. Some of the fertilizer washes into the Mississippi River and eventually flows into the Gulf of Mexico, promoting the growth of algae and endangering other aquatic life. a. Ammonium nitrate can be prepared by the following reaction: $$\mathrm{NH}_{3}(g)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{NH}_{4} \mathrm{NO}_{3}(a q)$$ How much nitric acid would be required to make the fertilizer needed for \(1 \mathrm{km}^{2}\) of cornfield per year? b. Ammonium ions dissolved in groundwater may be converted into \(\mathrm{NO}_{3}^{-}\) ions by bacterial action: $$\mathrm{NH}_{4}^{+}(a q)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{NO}_{3}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)+2 \mathrm{H}^{+}(a q)$$ If \(10 \%\) of the ammonium component of \(5.0 \times 10^{3}\) kilograms of fertilizer ends up as nitrate ions, how much oxygen would be consumed?

A reaction vessel contains equal masses of magnesium metal and oxygen gas. The mixture is ignited, forming MgO. After the reaction has gone to completion, the mass of the \(\mathrm{MgO}\) is less than the mass of the reactants. Is this result a violation of the law of conservation of mass? Explain your answer.

Syngas An industrial process for producing hydrogen gas is based on the reaction between carbon heated to incandescence and steam that produces a mixture of \(\mathrm{CO}\) and \(\mathrm{H}_{2}\) called synthesis gas, or syngas. a. Write a balanced chemical equation for the production of syngas. b. If a reaction vessel that initially contains 66 kilograms of incandescent carbon and excess steam produces \(6.8 \mathrm{kg}\) \(\mathrm{H}_{2},\) what is the percent yield?

Titanium dioxide and zinc oxide are common names of two of the active ingredients approved by the U.S. FDA for use in sunscreens. a. What are the chemical formulas of these compounds? b. What are the proper names of the compounds based on the rules for naming described in Chapter \(4 ?\) c. Which of the two compounds contains the higher percentage of oxygen by mass?
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