Textbook Question
Write the balanced chemical equation for the reaction of aqueous potassium hydroxide with aqueous iron(III) chloride to form solid iron(III) hydroxide and aqueous potassium chloride.
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Ch.4 - Chemical Reactions and Chemical Quantities
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 4, Problem 34c
Balance the equation and calculate how many moles of N2 form when each quantity of reactant completely reacts. N2H4(l) → NH3(g) + N2(g) c. 33.9 g N2H4
Verified step by step guidance1
Step 1: Write the unbalanced chemical equation: \( \text{N}_2\text{H}_4(l) \rightarrow \text{NH}_3(g) + \text{N}_2(g) \).
Step 2: Balance the chemical equation. Start by balancing the nitrogen atoms. Since there are 2 nitrogen atoms in \( \text{N}_2\text{H}_4 \), you need 2 \( \text{NH}_3 \) molecules to balance the nitrogen: \( \text{N}_2\text{H}_4(l) \rightarrow 2\text{NH}_3(g) + \text{N}_2(g) \).
Step 3: Check the balance of hydrogen atoms. \( \text{N}_2\text{H}_4 \) has 4 hydrogen atoms, and 2 \( \text{NH}_3 \) molecules have 6 hydrogen atoms. Adjust the equation to balance hydrogen: \( 3\text{N}_2\text{H}_4(l) \rightarrow 4\text{NH}_3(g) + 3\text{N}_2(g) \).
Step 4: Calculate the molar mass of \( \text{N}_2\text{H}_4 \) using the atomic masses: \( 2 \times 14.01 + 4 \times 1.01 = 32.05 \text{ g/mol} \).
Step 5: Convert 33.9 g of \( \text{N}_2\text{H}_4 \) to moles using its molar mass: \( \text{moles of } \text{N}_2\text{H}_4 = \frac{33.9 \text{ g}}{32.05 \text{ g/mol}} \). Use the balanced equation to find moles of \( \text{N}_2 \) produced: \( \text{moles of } \text{N}_2 = \frac{3}{3} \times \text{moles of } \text{N}_2\text{H}_4 \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. In the given reaction, balancing will help determine the stoichiometric relationships between the reactants and products.
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Balancing Chemical Equations
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced equations. It allows chemists to predict how much of a product will form from a given amount of reactant. In this case, stoichiometry will be used to calculate the moles of N2 produced from the given mass of N2H4, using the molar ratios derived from the balanced equation.
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Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between grams and moles in stoichiometric calculations. For N2H4, the molar mass must be calculated to convert the given mass (33.9 g) into moles, which will then be used to find the amount of N2 produced in the reaction.
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Related Practice
Textbook Question
Balance each chemical equation. b. Co(NO3)3(aq) + (NH4)2S(aq) → Co2S3(s) + NH4NO3(aq)
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Textbook Question
Consider the balanced equation:
SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g)
Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.
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Textbook Question
Balance the equation and calculate how many moles of O2 form when each quantity of reactant completely reacts. N2O5( g) → NO2(g) + O2(g) a. 1.2 mol N2O5
Textbook Question
Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr2(aq) + H2(g)
What mass of HBr (in g) do you need to dissolve a 2.80-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?
Textbook Question
Sulfuric acid dissolves aluminum metal according to the reaction:
2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
Suppose you want to dissolve an aluminum block with a mass of 11.3 g. What minimum mass of H2SO4 (in g) do you need? What mass of H2 gas (in g) does the complete reaction of the aluminum block produce?