Textbook Question
The reaction Fe3+(aq) + Cl-(aq) ⇌ FeCl2+(aq) is endothermic. How will the equilibrium concentration of FeCl2+ change when
b. Cl- is precipitated by addition of AgNO3?
2017
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Ch.7 Chemical Reactions: Energy, Rate and Equilibrium
McMurry8th EditionFundamentals of GOBISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
Chapter 7, Problem 69a
Magnetite, an iron ore with formula Fe3O4, can be reduced by treatment with hydrogen to yield iron metal and water vapor.
a. Write the balanced equation.
Verified step by step guidance1
Step 1: Write the unbalanced chemical equation for the reaction. The reactants are magnetite (Fe₃O₄) and hydrogen gas (H₂), and the products are iron metal (Fe) and water vapor (H₂O). The unbalanced equation is: Fe₃O₄ + H₂ → Fe + H₂O.
Step 2: Balance the iron (Fe) atoms. Magnetite contains 3 iron atoms, so place a coefficient of 3 in front of Fe on the product side: Fe₃O₄ + H₂ → 3Fe + H₂O.
Step 3: Balance the oxygen (O) atoms. Magnetite contains 4 oxygen atoms, and water contains 1 oxygen atom per molecule. Place a coefficient of 4 in front of H₂O on the product side: Fe₃O₄ + H₂ → 3Fe + 4H₂O.
Step 4: Balance the hydrogen (H) atoms. There are 8 hydrogen atoms on the product side (from 4H₂O), so place a coefficient of 4 in front of H₂ on the reactant side: Fe₃O₄ + 4H₂ → 3Fe + 4H₂O.
Step 5: Verify that the equation is balanced. Check that the number of each type of atom is the same on both sides of the equation: 3 Fe, 4 O, and 8 H. The balanced equation is: Fe₃O₄ + 4H₂ → 3Fe + 4H₂O.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reduction Reaction
A reduction reaction involves the gain of electrons or a decrease in oxidation state by a substance. In the context of magnetite (Fe3O4) being treated with hydrogen, the iron ions in the ore are reduced to elemental iron, while hydrogen is oxidized to water vapor. Understanding this concept is crucial for balancing the chemical equation correctly.
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Reduction Reactions Concept 1
Balancing Chemical Equations
Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is achieved by adjusting the coefficients of the reactants and products. In the case of the reduction of magnetite, it is essential to balance the iron, hydrogen, and oxygen atoms to accurately represent the reaction.
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Stoichiometry
Stoichiometry is the study of the quantitative relationships between the amounts of reactants and products in a chemical reaction. It allows chemists to predict how much product can be formed from given amounts of reactants. In this scenario, understanding stoichiometry helps in determining the correct ratios of magnetite and hydrogen needed to produce iron and water vapor.
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Related Practice
Textbook Question
For the unbalanced combustion reaction shown, 1 mol of ethanol, C2H5OH, releases 327 kcal (1370 kJ):
C2H5OH + O2 → CO2 + H2O
e. If the density of ethanol is 0.789 g/mL, calculate the combustion energy of ethanol in kilocalories/milliliter and kilojoules/milliliter
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Textbook Question
For the production of ammonia from its elements, ∆H = -22 kcal/mol(-19 kJ/mol).
b. How much energy (in kilocalories and kilojoules) is involved in the production of 0.700 mol of NH3?
1503
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Textbook Question
Magnetite, an iron ore with formula Fe3O4, can be reduced by treatment with hydrogen to yield iron metal and water vapor.
d. This reaction has K = 2.3 × 10-18. Are the reactants or the products favored?
2277
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Textbook Question
For the evaporation of water, H2O(l) → H2O(g), at 100°C, ∆H = +9.72 kcal/mol (+40.7 kJ/mol).
b. How many kilojoules are released when 10.0 g of H2O(g) is condensed?
3274
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Textbook Question
Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor:
NH3(g) + O2(g) ⇌ NO(g) + H2O(g) + Heat
b. Write the equilibrium equation.
2897
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