Domanda del libro di testo
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
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 4, Problema 27a
Calculate how many moles of NO2 form when each quantity of reactant completely reacts. 2 N2O5( g) → 4 NO2(g) + O2(g) a. 2.5 mol N2O5
Guida verificata passo dopo passo1
Start by identifying the balanced chemical equation: 2 \(\text{N}\)_2\(\text{O}\)_5 (g) \(\rightarrow\) 4 \(\text{NO}\)_2 (g) + \(\text{O}\)_2 (g)
Determine the mole ratio between \(\text{N}\)_2\(\text{O}\)_5 and \(\text{NO}\)_2 from the balanced equation. The ratio is 2:4, which simplifies to 1:2.
Use the mole ratio to set up a conversion factor. For every 1 mole of \(\text{N}\)_2\(\text{O}\)_5, 2 moles of \(\text{NO}\)_2 are produced.
Multiply the given moles of \(\text{N}\)_2\(\text{O}\)_5 by the conversion factor to find the moles of \(\text{NO}\)_2.
Perform the calculation: 2.5 \(\text{ mol N}\)_2\(\text{O}\)_5 \(\times\) \(\frac{2 \text{ mol NO}\)_2}{1 \(\text{ mol N}\)_2\(\text{O}\)_5}.
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Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows chemists to predict how much of each substance will be produced or consumed based on balanced chemical equations. In this case, the stoichiometric coefficients from the balanced equation indicate that 2 moles of N2O5 produce 4 moles of NO2.
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Percorso guidato
01:16
Stoichiometry Concept
Mole Concept
The mole concept is a fundamental principle in chemistry that defines the amount of substance. One mole is equivalent to 6.022 x 10^23 entities (atoms, molecules, etc.). This concept is crucial for converting between grams and moles, allowing for calculations of how many moles of products can be formed from a given number of moles of reactants.
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01:25Mole Concept
Balanced Chemical Equation
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It ensures the law of conservation of mass is upheld. In the provided reaction, the balanced equation shows that 2 moles of N2O5 yield 4 moles of NO2, which is essential for determining the amount of NO2 produced from a specific quantity of N2O5.
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Percorso guidato
01:32Balancing Chemical Equations
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Calculate how many moles of NH3 form when each quantity of reactant completely reacts. 3 N2H4(l) → 4 NH3(g) + N2(g) c. 65.3 g N2H4
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