Domanda del libro di testo
Consider the following reaction: 2 NO1g2 + 2 H21g2¡N21g2 + 2 H2O1g2 (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and 3H24 is increased to 0.030 M?
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Ch.14 - Chemical Kinetics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 32a
The reaction between ethyl bromide (C2H5Br) and hydroxide ion in ethyl alcohol at 330 K, C2H5Br(alc) + OH-(alc) → C2H5OH(l) + Br-(alc), is first order each in ethyl bromide and hydroxide ion. When [C2H5Br] is 0.0477 M and [OH-] is 0.100 M, the rate of disappearance of ethyl bromide is 1.7×10-7 M/s. (a) What is the value of the rate constant?
Guida verificata passo dopo passo1
Identify the rate law expression based on the given reaction order. Since the reaction is first order in both ethyl bromide and hydroxide ion, the rate law can be expressed as: Rate = k [C2H5Br][OH-].
Substitute the given concentrations and the rate of disappearance into the rate law expression. Here, [C2H5Br] = 0.0477 M, [OH-] = 0.100 M, and Rate = 1.7 * 10^-7 M/s.
Rearrange the rate law equation to solve for the rate constant k. This can be done by dividing both sides of the equation by the product of the concentrations of the reactants: k = Rate / ([C2H5Br][OH-]).
Plug the values into the rearranged equation to find the value of k. Ensure that all units are consistent for concentration (M) and time (s).
The calculated value of k will be in units of M^-1s^-1, which is appropriate given the reaction order and the units of the rate and concentrations.
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Rate Law
The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. For a reaction that is first order in each reactant, the rate can be described by the equation: Rate = k[C2H5Br][OH-], where k is the rate constant. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.
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Percorso guidato
01:52
Rate Law Fundamentals
First-Order Reactions
A first-order reaction is one where the rate is directly proportional to the concentration of one reactant. In this case, both ethyl bromide and hydroxide ion are first-order, meaning that doubling their concentrations will double the reaction rate. This concept is crucial for calculating the rate constant from the given rate and concentrations.
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02:29First-Order Reactions
Rate Constant (k)
The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a specific temperature. It provides insight into the speed of the reaction; a larger k indicates a faster reaction. To find k, one can rearrange the rate law equation using the provided rate and concentrations, which is key to solving the problem.
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Percorso guidato
01:14Equilibrium Constant K
Pratica correlata
Domanda del libro di testo
The reaction between ethyl bromide (C2H5Br) and hydroxide ion in ethyl alcohol at 330 K, C2H5Br(alc) + OH-(alc) → C2H5OH(l) + Br-(alc), is first order each in ethyl bromide and hydroxide ion. When [C2H5Br] is 0.0477 M and [OH-] is 0.100 M, the rate of disappearance of ethyl bromide is 1.7×10-7 M/s. (b) What are the units of the rate constant?
Domanda del libro di testo
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:
[OCl4-] (M) [I-] (M) Initial Rate (M,s)
1.5 * 10-3 1.5 * 10-3
1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4
1.5 * 10-3 3.0 * 10-3 2.72 * 10-4
(a) Write the rate law for this reaction.
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Domanda del libro di testo
The reaction between ethyl bromide (C2H5Br) and hydroxide ion in ethyl alcohol at 330 K, C2H5Br(alc) + OH-(alc) → C2H5OH(l) + Br-(alc), is first order each in ethyl bromide and hydroxide ion. When [C2H5Br] is 0.0477 M and [OH-] is 0.100 M, the rate of disappearance of ethyl bromide is 1.7×10-7 M/s. (c) How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution?
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Domanda del libro di testo
Consider the following reaction:
2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
(b) If the rate constant for this reaction at 1000 K is 6.0 × 104 M-2 s-1, what is the reaction rate when [NO] = 0.035 M and [H2] = 0.015 M?
(c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H2 is 0.010 M?