Textbook Question
From a plot of the concentration–time data in Worked Example 14.9, estimate: (b) the initial rate of decomposition of NO2.
Ch.14 - Chemical Kinetics
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 14, Problem 54b
From the plot of concentration–time data in Figure 14.1, estimate: (b) the initial rate of decomposition of N2O5.
Verified step by step guidance1
Identify the initial concentration of N2O5 from the plot at time t = 0.
Find the concentration of N2O5 at a small time interval after t = 0 from the plot.
Calculate the change in concentration, Δ[N2O5], by subtracting the initial concentration from the concentration at the chosen small time interval.
Determine the change in time, Δt, which is the time interval chosen in step 2.
Calculate the initial rate of decomposition of N2O5 using the formula: Rate = -Δ[N2O5]/Δt. The negative sign indicates the concentration of N2O5 is decreasing.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Rate of Reaction
The rate of reaction refers to the speed at which reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product per unit time. Understanding how to calculate and interpret reaction rates is essential for analyzing concentration-time data.
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Average Rate of Reaction
Concentration-Time Graphs
Concentration-time graphs visually represent how the concentration of a reactant or product changes over time. The slope of the curve at any point indicates the rate of reaction at that moment. For estimating initial rates, one typically examines the slope of the curve at the very beginning of the reaction, where the concentration changes most rapidly.
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Decomposition Reactions
Decomposition reactions involve the breakdown of a compound into simpler substances, often resulting in the release of gases. In the case of N2O5, its decomposition can be represented by a specific reaction equation. Understanding the nature of decomposition reactions helps in predicting the behavior of reactants and products over time.
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Related Practice
Textbook Question
Draw a plausible transition state for the bimolecular reaction of nitric oxide with ozone. Use dashed lines to indicate the atoms that are weakly linked together in the transition state. NO(g) + O3(g) NO2(g) + O2(g)
Textbook Question
Ammonia is manufactured in large amounts by the reaction N21g2 + 3 H21g2S 2 NH31g2 (b) How is the rate of formation of NH3 related to the rate of consumption of N2?
Textbook Question
From a plot of the concentration–time data in Worked Example 14.9, estimate: (a) the instantaneous rate of decomposition of NO2 at t = 100 s.
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Textbook Question
From the plot of concentration–time data in Figure 14.1, estimate: (a) the instantaneous rate of decomposition of N2O5 at t = 200 s.
Textbook Question
Use the information in Table 14.1 and Figure 14.1 to estimate the instantaneous rate of appearance of NO2 at t = 350 s by calculating the average rate of appearance of NO2 over the following time intervals centered on t = 350 s. (a) 0 to 700 s (b) 100 to 600 s (c) 200 to 500 s (d) 300 to 400 s Which is the best estimate, and why?