Domanda del libro di testo
Consider the reaction:
2 HBr (g) → H2 (g) + Br2 (g)
c. If the volume of the reaction vessel in part b was 1.50 L, what amount of Br2 (in moles) was formed during the first 15.0 s of the reaction?
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Ch.14 - Chemical Kinetics
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
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Capitolo 14, Problema 25a
Consider the reaction:
2 HBr (g) → H2 (g) + Br2 (g)
a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.
Guida verificata passo dopo passo1
Express the rate of the reaction in terms of the change in concentration of HBr. The rate of disappearance of HBr can be written as: \( -\frac{1}{2} \frac{\Delta [\text{HBr}]}{\Delta t} \).
Express the rate of the reaction in terms of the change in concentration of H2. The rate of formation of H2 can be written as: \( \frac{\Delta [\text{H}_2]}{\Delta t} \).
Express the rate of the reaction in terms of the change in concentration of Br2. The rate of formation of Br2 can be written as: \( \frac{\Delta [\text{Br}_2]}{\Delta t} \).
Since the stoichiometry of the reaction is 2:1:1 for HBr, H2, and Br2 respectively, the rate of disappearance of HBr is twice the rate of formation of H2 and Br2.
Therefore, the rate of the reaction can be expressed as: \( -\frac{1}{2} \frac{\Delta [\text{HBr}]}{\Delta t} = \frac{\Delta [\text{H}_2]}{\Delta t} = \frac{\Delta [\text{Br}_2]}{\Delta t} \).
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Reaction Rate
The reaction rate is a measure of how quickly reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product over time. In this case, the rate can be defined in terms of the decrease in concentration of HBr and the increase in concentrations of H2 and Br2.
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Average Rate of Reaction
Stoichiometry
Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction, based on the balanced chemical equation. For the given reaction, the coefficients indicate that two moles of HBr produce one mole of H2 and one mole of Br2, which is essential for expressing the rates in terms of their respective concentrations.
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01:16Stoichiometry Concept
Concentration Change
Concentration change refers to the difference in the amount of a substance in a given volume over time. In the context of the reaction, it is important to express how the concentrations of HBr, H2, and Br2 change as the reaction progresses, which is crucial for calculating the rate of the reaction accurately.
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01:53Chemical Changes