Textbook Question
From the plot of concentration–time data in Figure 14.1, estimate: (b) the initial rate of decomposition of N2O5.
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 52
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?
Verified step by step guidance1
Identify the concentration of NO2 at the given time intervals from Table 14.1 and Figure 14.1.
Calculate the average rate of appearance of NO2 for each interval using the formula: \( \text{Average Rate} = \frac{[\text{NO}_2]_\text{final} - [\text{NO}_2]_\text{initial}}{t_\text{final} - t_\text{initial}} \).
For interval (a) 0 to 700 s, use the concentrations at 0 s and 700 s to find the average rate.
For interval (b) 100 to 600 s, use the concentrations at 100 s and 600 s to find the average rate.
Compare the average rates calculated for each interval to determine which is closest to the instantaneous rate at t = 350 s, considering that shorter intervals around 350 s provide a better estimate.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Instantaneous Rate vs. Average Rate
The instantaneous rate of a reaction refers to the rate at a specific moment in time, while the average rate is calculated over a defined time interval. To estimate the instantaneous rate at t = 350 s, one can analyze the average rates over various intervals that include this time point. Understanding the difference between these rates is crucial for accurately interpreting the data.
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01:30
Instantaneous Rate
Rate of Reaction
The rate of reaction quantifies how quickly reactants are converted into products. It can be expressed in terms of the change in concentration of a reactant or product over time. In this case, the focus is on the appearance of NO2, which requires calculating the change in its concentration over the specified time intervals to determine the rate.
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Data Interpretation from Graphs and Tables
Interpreting data from tables and graphs is essential for estimating rates of reaction. Table 14.1 likely provides concentration values at various times, while Figure 14.1 may illustrate the concentration changes graphically. Understanding how to extract and analyze this information allows for accurate calculations of average rates over the specified intervals.
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Related Practice
Textbook Question
Consider a reaction that occurs by the following mechanism:
A + BC → AC + B
AC + D → A + CD
The potential energy profile for this reaction is as follows:
(c) Which of the two steps in the mechanism is the rate-determining step? Write the rate law for the overall reaction.
Textbook Question
Consider a reaction that occurs by the following mechanism:
A + BC → AC + B
AC + D → A + CD
The potential energy profile for this reaction is as follows:
(d) Is the reaction endothermic or exothermic? Add labels to the diagram that show the values of the energy of reaction ΔE and the activation energy Ea for the overall reaction.
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
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
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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