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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.14 - Chemical KineticsProblema 46
Capitolo 14, Problema 46

From the following data for the first-order gas-phase isomerization of CH3NC to CH3CN at 215°C, calculate the first-order rate constant and half-life for the reaction:
Time (s) Pressure CH3NC (torr)
0 502
2000 335
5000 180
8000 95.5
12,000 41.7
15,000 22.4

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1
Identify that the reaction is a first-order reaction, which means the rate law is given by \( \ln [A]_t = -kt + \ln [A]_0 \), where \([A]_t\) is the concentration (or pressure) at time \(t\), \([A]_0\) is the initial concentration (or pressure), and \(k\) is the rate constant.
Use the data provided to calculate the rate constant \(k\). Choose two data points, for example, at \(t = 0\) and \(t = 2000\) seconds. Substitute these values into the first-order rate equation: \( \ln(335) = -k(2000) + \ln(502) \).
Rearrange the equation to solve for \(k\): \( k = \frac{\ln(502) - \ln(335)}{2000} \).
Calculate the half-life of the reaction using the formula for the half-life of a first-order reaction: \( t_{1/2} = \frac{0.693}{k} \).
Verify the consistency of the calculated rate constant \(k\) by using another set of data points, such as \(t = 5000\) and \(t = 8000\), and check if the calculated \(k\) is approximately the same.

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First-Order Reactions

First-order reactions are chemical reactions where the rate is directly proportional to the concentration of one reactant. This means that as the concentration of the reactant decreases, the rate of the reaction also decreases. The rate law for a first-order reaction can be expressed as rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.
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First-Order Reactions

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate equation that is specific to a given reaction at a particular temperature. For first-order reactions, the rate constant can be determined using the integrated rate law, which relates the concentration of the reactant to time. The units of k for a first-order reaction are typically s⁻¹.
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Equilibrium Constant K

Half-Life (t1/2)

The half-life of a reaction is the time required for the concentration of a reactant to decrease to half of its initial value. For first-order reactions, the half-life is constant and does not depend on the initial concentration, calculated using the formula t1/2 = 0.693/k. This property is useful for predicting how long it will take for a reaction to reach a certain extent of completion.
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Zero-Order Half-life
Pratica correlata
Domanda del libro di testo

The first-order rate constant for the decomposition of N2O5, 2 N2O5(g) → 4 NO2(g) + O2(g), at 70°C is 6.82×10-3 s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 2.0 L. (c) What is the half-life of N2O5 at 70°C?

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Domanda del libro di testo

The first-order rate constant for the decomposition of N2O5, 2 N2O5(g) → 4 NO2(g) + O2(g), at 70°C is 6.82×10-3 s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 2.0 L. (a) How many moles of N2O5 will remain after 5.0 min?

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Domanda del libro di testo

Consider the data presented in Exercise 14.19. (a) By using appropriate graphs, determine whether the reaction is first order or second order.

Domanda del libro di testo

Consider the data presented in Exercise 14.19. (c) What is the half-life for the reaction?

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