Domanda del libro di testo
A reaction A + B → C obeys the following rate law: Rate = k[B]2. (a) If [A] is doubled, how will the rate change? Will the rate constant change?
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Ch.14 - Chemical Kinetics
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 28a
Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (a) Write the rate law for the reaction.
Guida verificata passo dopo passo1
insert step 1> Identify the order of the reaction with respect to each reactant. The problem states that the reaction is first order in A, zero order in B, and second order in C.
insert step 2> Recall that the rate law for a reaction is expressed as: \( \text{Rate} = k[A]^m[B]^n[C]^p \), where \( k \) is the rate constant, and \( m, n, \) and \( p \) are the orders of the reaction with respect to A, B, and C, respectively.
insert step 3> Substitute the given orders into the rate law expression: \( m = 1 \), \( n = 0 \), and \( p = 2 \).
insert step 4> Write the rate law using the substituted values: \( \text{Rate} = k[A]^1[B]^0[C]^2 \).
insert step 5> Simplify the rate law expression by removing any terms raised to the power of zero, as they equal 1: \( \text{Rate} = k[A][C]^2 \).
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Rate Law
The rate law of a chemical reaction expresses the relationship between the rate of the reaction and the concentration of its reactants. It is typically formulated as an equation where the rate is proportional to the concentrations of the reactants raised to their respective orders. The order of a reactant indicates how the rate is affected by changes in its concentration.
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Percorso guidato
01:52
Rate Law Fundamentals
Reaction Order
Reaction order refers to the exponent to which the concentration of a reactant is raised in the rate law. It can be determined experimentally and indicates the sensitivity of the reaction rate to changes in that reactant's concentration. In this case, the reaction is first order in A, zero order in B, and second order in C, meaning the rate depends linearly on A, is independent of B, and depends quadratically on C.
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Percorso guidato
00:36Average Bond Order
Units of Rate Constant
The units of the rate constant (k) in a rate law depend on the overall order of the reaction. For a reaction that is first order in A, zero order in B, and second order in C, the overall order is 3 (1 + 0 + 2). The units of k for this reaction would be M^-2 s^-1, where M is molarity, reflecting how the rate of reaction changes with the concentrations of the reactants.
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00:45Rate Constant Units
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