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
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 30b,c
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?
Guida verificata passo dopo passo1
Identify the rate law for the given reaction. Since the reaction is 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g), the rate law can be expressed as: rate = k[NO]^2[H2]^2, where k is the rate constant.
For part (b), substitute the given values into the rate law. Use k = 6.0 × 10^4 M^-2 s^-1, [NO] = 0.035 M, and [H2] = 0.015 M. The expression becomes: rate = (6.0 × 10^4 M^-2 s^-1) × (0.035 M)^2 × (0.015 M)^2.
Calculate the rate for part (b) by evaluating the expression from the previous step. This involves squaring the concentrations of NO and H2, multiplying them together, and then multiplying by the rate constant.
For part (c), substitute the new concentration values into the rate law. Use k = 6.0 × 10^4 M^-2 s^-1, [NO] = 0.10 M, and [H2] = 0.010 M. The expression becomes: rate = (6.0 × 10^4 M^-2 s^-1) × (0.10 M)^2 × (0.010 M)^2.
Calculate the rate for part (c) by evaluating the expression from the previous step. This involves squaring the new concentrations of NO and H2, multiplying them together, and then multiplying by the rate constant.
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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 of the form aA + bB → products, the rate can be described by the equation Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B, respectively. Understanding the rate law is essential for calculating reaction rates based on varying concentrations.
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Percorso guidato
01:52
Rate Law Fundamentals
Order of Reaction
The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. It indicates how the rate of reaction is affected by the concentration of that reactant. For example, if the reaction is first order with respect to NO, doubling the concentration of NO will double the reaction rate. Identifying the order of each reactant is crucial for accurately determining the overall reaction rate.
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Percorso guidato
00:36Average Bond Order
Units of Rate Constant
The units of the rate constant (k) depend on the overall order of the reaction. For a second-order reaction, like the one given (2 NO + 2 H2 → N2 + 2 H2O), the units of k are M^-2 s^-1. This means that the rate of reaction is proportional to the product of the concentrations of the reactants raised to their respective orders. Understanding these units is vital for correctly applying the rate law to calculate reaction rates.
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Percorso guidato
00:45Rate Constant Units
Pratica correlata
Domanda del libro di testo
The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 → 4 NO2 + O2. The rate law is first order in N2O5. At 64°C the rate constant is 4.82 × 10-3 s-1. (c) What happens to the rate when the concentration of N2O5 is doubled to 0.0480 M? (d) What happens to the rate when the concentration of N2O5 is halved to 0.0120 M?
Domanda del libro di testo
The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 → 4 NO2 + O2. The rate law is first order in N2O5. At 64°C the rate constant is 4.82 × 10-3 s-1. (a) Write the rate law for the reaction.
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Domanda del libro di testo
Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (e) By what factor does the rate change when the concentrations of all three reactants are tripled?
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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. (a) What is the value of the rate constant?
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