Textbook Question
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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Table of contents
- 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: 9780134414232Not the one you use?Change textbook
Chapter 14, Problem 26
(b) The rate of decrease in N2H4 partial pressure in a closed reaction vessel from the reaction N2H4(g) + H2(g) → 2 NH3(g) is 74 torr per hour. What are the rates of change of NH3 partial pressure and total pressure in the vessel?
Verified step by step guidance1
Identify the stoichiometry of the reaction: N2H4(g) + H2(g) → 2 NH3(g). This tells us that 1 mole of N2H4 reacts with 1 mole of H2 to produce 2 moles of NH3.
Recognize that the rate of decrease in N2H4 partial pressure is given as 74 torr per hour. According to the stoichiometry, for every mole of N2H4 that reacts, 2 moles of NH3 are produced.
Calculate the rate of increase in NH3 partial pressure. Since 2 moles of NH3 are produced for every mole of N2H4 that reacts, the rate of increase in NH3 partial pressure is twice the rate of decrease in N2H4 partial pressure.
Determine the rate of change of total pressure in the vessel. The total pressure change is the sum of the changes in partial pressures of all gases involved. Consider the stoichiometry and the fact that H2 is consumed and NH3 is produced.
Apply the concept of partial pressures and stoichiometry to find the net change in total pressure. Since 1 mole of N2H4 and 1 mole of H2 produce 2 moles of NH3, calculate the net change in moles of gas and relate it to the change in total pressure.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. In this case, the stoichiometric coefficients indicate that one mole of hydrazine (N2H4) produces two moles of ammonia (NH3). Understanding these ratios is essential for determining the rates of change of the substances involved in the reaction.
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Guided course
01:16
Stoichiometry Concept
Rate of Reaction
The rate of reaction refers to the speed at which reactants are converted into products. It can be expressed in terms of the change in concentration or partial pressure of a substance over time. In this scenario, knowing the rate of decrease of N2H4 allows us to calculate the corresponding increase in NH3 and the total pressure change in the vessel.
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Guided course
02:03Average Rate of Reaction
Total Pressure in a Closed System
In a closed system, the total pressure is the sum of the partial pressures of all gases present. According to Dalton's Law of Partial Pressures, changes in the partial pressures of individual gases will affect the total pressure. By calculating the change in NH3's partial pressure, we can determine how the total pressure in the vessel is affected by the reaction.
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02:09Total Pressure Example
Related Practice
Textbook Question
For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant:
(a) 2 H2O(g) → 2 H2(g) + O2(g)
(b) 2 SO2(g) + O2(g) → 2 SO3(g)
(c) 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
(d) N2(g) + 2 H2(g) → N2H4(g)
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Textbook Question
A reaction A + B → C obeys the following rate law: Rate = k[B]2. (c) What are the units of the rate constant?
Textbook Question
(b) The reaction 2 NO1g2 + Cl21g2¡2 NOCl1g2 is carried out in a closed vessel. If the partial pressure of NO is decreasing at the rate of 56 torr/min, what is the rate of change of the total pressure of the vessel?
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Textbook Question
A reaction A + B → C obeys the following rate law: Rate = k[B]2. (b) What are the reaction orders for A and B? What is the overall reaction order?
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Textbook Question
(a) Consider the combustion of hydrogen, 2 H21g2 + O21g2 ¡ 2 H2O1g2. If hydrogen is burning at the rate of 0.48 mol>s, what is the rate of consumption of oxygen? What is the rate of formation of water vapor?
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