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 29c,d
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?
Guida verificata passo dopo passo1
Identify the rate law for the reaction. Since the reaction is first order in N2O5, the rate law can be expressed as: rate = k[N2O5], where k is the rate constant.
For part (c), when the concentration of N2O5 is doubled to 0.0480 M, substitute this new concentration into the rate law: rate = k[0.0480 M].
Since the rate law is first order, doubling the concentration of N2O5 will double the rate of the reaction. This is because the rate is directly proportional to the concentration of N2O5.
For part (d), when the concentration of N2O5 is halved to 0.0120 M, substitute this new concentration into the rate law: rate = k[0.0120 M].
Halving the concentration of N2O5 will halve the rate of the reaction, as the rate is directly proportional to the concentration of N2O5 in a first-order reaction.
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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 first-order reaction, the rate is directly proportional to the concentration of the reactant raised to the first power. This means that if the concentration of the reactant is doubled, the rate of the reaction also doubles, while halving the concentration will halve the rate.
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Percorso guidato
01:52
Rate Law Fundamentals
First-Order Reaction
A first-order reaction is one where the rate of reaction depends linearly on the concentration of one reactant. In this case, the rate constant (k) remains constant, and the reaction rate can be expressed as rate = k[N2O5]. This characteristic allows for straightforward predictions about how changes in concentration affect the reaction rate.
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02:29First-Order Reactions
Concentration and Reaction Rate
Concentration refers to the amount of a substance in a given volume. In chemical kinetics, changes in concentration directly influence the rate of reaction. For first-order reactions, increasing the concentration of the reactant increases the rate proportionally, while decreasing the concentration reduces the rate, allowing for predictable calculations based on concentration changes.
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02:03Average Rate of Reaction
Pratica correlata
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. (b) How does the rate change when [A] is doubled and the other reactant concentrations are held constant? (c) How does the rate change when [B] is tripled and the other reactant concentrations are held constant? (d) How does the rate change when [C] is tripled and the other reactant concentrations are held constant? (f) By what factor does the rate change when the concentrations of all three reactants are cut in half?
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
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?