MASTERING CHEMISTY NVCC ACCESS CODE
1st Edition
ISBN: 9780136444459
Author: Tro
Publisher: PEARSON
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Textbook Question
Chapter 14, Problem 12E
Write integrated rate laws for zero-order, first-order, and second-order reactions of the form
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Chapter 14 Solutions
MASTERING CHEMISTY NVCC ACCESS CODE
Ch. 14 - Explain why lizards become sluggish in cold...Ch. 14 - Why are reaction rates important (both practically...Ch. 14 - Using the idea that reactions occur as a result of...Ch. 14 - Using the idea that reactions occur as a result of...Ch. 14 - What units are typically used to express the rate...Ch. 14 - Why is the reaction rate for reactants defined as...Ch. 14 - Explain the difference between the average rate of...Ch. 14 - Consider a simple reaction in which a reactant A...Ch. 14 - How is the order of a reaction generally...Ch. 14 - For a reaction with multiple reactants, how is the...
Ch. 14 - Explain the difference between the rate law for a...Ch. 14 - Write integrated rate laws for zero-order,...Ch. 14 - What does the term half-life mean? Write the...Ch. 14 - How do reaction rates typically depend on...Ch. 14 - Prob. 15ECh. 14 - What is an Arrhenius plot? Explain the...Ch. 14 - Explain the meaning of the orientation factor in...Ch. 14 - Explain the difference between a normal chemical...Ch. 14 - In a reaction mechanism, what is an elementary...Ch. 14 - What are the two requirements for a proposed...Ch. 14 - What is an intermediate within a reaction...Ch. 14 - What is a catalyst? How does a catalyst increase...Ch. 14 - Explain the difference between homogeneous...Ch. 14 - What are the four basic steps involved in...Ch. 14 - What are enzymes? What is the active site of an...Ch. 14 - What is the general two-step mechanism by which...Ch. 14 - Consider the reaction. 2HBr(g)H2(g)+Br2(g) Express...Ch. 14 - Consider the reaction 2N2O(g)2N2(g)+O2(g) Express...Ch. 14 - For the reaction 2A(g)+B(g)3C(g) determine the...Ch. 14 - For the reaction A(g)+12B(g)2C(g) determine the...Ch. 14 - Consider the reaction. Cl2(g)+3F2(g)2ClF3(g)...Ch. 14 - Consider the reaction. 8H2S(g)+4O2(g)8H2O(g)+S8(g)...Ch. 14 - Consider the reaction: C4H8(g)2C2H4(g) The...Ch. 14 - Consider the reaction: NO2(g)NO(g)+12O2(g) The...Ch. 14 - Consider the reaction. H2(g)+Br2(g)2HBr(g) The...Ch. 14 - Consider the reaction. 2H2O2(aq)2H2O(l)+O2(g) The...Ch. 14 - This graph shows a plot of the rate of a reaction...Ch. 14 - This graph shows a plot of the rate of a reaction...Ch. 14 - What are the units of k for each type of reaction?...Ch. 14 - This reaction is first order in N2O5:...Ch. 14 - A reaction in which A, B, and C react to form...Ch. 14 - A reaction in which A, B, and C react to form...Ch. 14 - Consider the tabulated data showing initial rate...Ch. 14 - Consider the tabulated data showing initial rate...Ch. 14 - The tabulated data were collected for this...Ch. 14 - The tabulated data were collected for this...Ch. 14 - Indicate the order of reaction consistent with...Ch. 14 - Indicate the order of reaction consistent with...Ch. 14 - The tabulated data show the concentration of AB...Ch. 14 - The tabulated data show the concentration of N2O5...Ch. 14 - The tabulated data show the concentration of...Ch. 14 - Prob. 52ECh. 14 - This reaction was monitored as a function of time:...Ch. 14 - This reaction was monitored as a function of time:...Ch. 14 - Prob. 55ECh. 14 - Prob. 56ECh. 14 - Prob. 57ECh. 14 - Prob. 58ECh. 14 - The diagram shows the energy of a reaction as the...Ch. 14 - Prob. 60ECh. 14 - Prob. 61ECh. 14 - Prob. 62ECh. 14 - Prob. 63ECh. 14 - The rate constant (k) for a reaction is measured...Ch. 14 - The tabulated data shown here were collected for...Ch. 14 - Prob. 66ECh. 14 - The tabulated data were collected for the...Ch. 14 - Prob. 68ECh. 14 - A reaction has a rate constant of 0.0117/s at...Ch. 14 - A reaction has a rate constant of 0.000122/s at...Ch. 14 - Prob. 71ECh. 14 - Prob. 72ECh. 14 - Prob. 73ECh. 14 - Prob. 74ECh. 14 - Prob. 75ECh. 14 - Prob. 76ECh. 14 - Consider this three-step mechanism for a...Ch. 14 - Prob. 78ECh. 14 - Prob. 79ECh. 14 - Prob. 80ECh. 14 - Suppose that a catalyst lowers the activation...Ch. 14 - The activation barrier for the hydrolysis of...Ch. 14 - The tabulated data were collected for this...Ch. 14 - Prob. 84ECh. 14 - Consider the reaction: A+B+CD The rate law for...Ch. 14 - Consider the reaction: 2O3(g)3O2(g) The rate law...Ch. 14 - At 700 K acetaldehyde decomposes in the gas phase...Ch. 14 - Prob. 88ECh. 14 - Dinitrogen pentoxide decomposes in the gas phase...Ch. 14 - Cyclopropane (C3H6) reacts to form propene (C3H6)...Ch. 14 - Iodine atoms combine to form I2 in liquid hexane...Ch. 14 - Prob. 92ECh. 14 - The reaction AB(aq)A(g)+B(g) is second order in AB...Ch. 14 - The reaction 2H2O2(aq)2H2O(l)+O2(g) is first order...Ch. 14 - Consider this energy diagram: a. How many...Ch. 14 - Consider the reaction in which HCI adds across the...Ch. 14 - The desorption of a single molecular layer of...Ch. 14 - The evaporation of a 120-nm film of n-pentane from...Ch. 14 - Prob. 99ECh. 14 - Prob. 100ECh. 14 - Prob. 101ECh. 14 - Consider the two reactions: O+N2NO+NEa= 315 kJ/mol...Ch. 14 - Anthropologists can estimate the age of a bone or...Ch. 14 - Prob. 104ECh. 14 - Consider the gas-phase reaction: H2(g)+I2(g)2HI(g)...Ch. 14 - Consider the reaction:...Ch. 14 - Prob. 107ECh. 14 - Prob. 108ECh. 14 - A certain substance X decomposes. Fifty percent of...Ch. 14 - Prob. 110ECh. 14 - Prob. 111ECh. 14 - Prob. 112ECh. 14 - Prob. 113ECh. 14 - Prob. 114ECh. 14 - Prob. 115ECh. 14 - Prob. 116ECh. 14 - Phosgene (Cl2CO), a poison gas used in World War...Ch. 14 - The rate of decomposition of N2O3(g) to NO2(g) and...Ch. 14 - At 473 K, for the elementary reaction...Ch. 14 - Prob. 120ECh. 14 - Prob. 121ECh. 14 - A particular reaction, Aproducts has a rate that...Ch. 14 - Prob. 123ECh. 14 - A certain compound, A, reacts to form products...Ch. 14 - Methane (CH4) is a greenhouse gas emitted by...Ch. 14 - This graph shows the concentration of the reactant...Ch. 14 - Prob. 2SAQCh. 14 - Prob. 3SAQCh. 14 - Prob. 4SAQCh. 14 - Prob. 5SAQCh. 14 - Prob. 6SAQCh. 14 - Prob. 7SAQCh. 14 - Prob. 8SAQCh. 14 - The rate constant of a reaction is measured at...Ch. 14 - Prob. 10SAQCh. 14 - The mechanism shown here is proposed for the...Ch. 14 - Prob. 12SAQCh. 14 - These images represent the first-order reaction AB...Ch. 14 - Prob. 14SAQCh. 14 - Prob. 15SAQ
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- Explain how a species might be part of a rate law but not part of a balanced chemical reaction.arrow_forward. find the rate law predicted for a particular reaction mechanism.arrow_forwardOne experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?arrow_forward
- Gaseous azomethane (CH3N2CH3) decomposes to ethane and nitrogen when heated: CH3N2CH3(g) CH3CH3(g) + N2(g) The decomposition of azomethane is a first-order reaction with k = 3.6 104 s1 at 600 K. (a) A sample of gaseous CH3N2CH3 is placed in a flask and heated at 600 K for 150 seconds. What fraction of the initial sample remains after this time? (b) How long must a sample be heated so that 99% of the sample has decomposed?arrow_forwardExplain why half-lives are not normally used to describe reactions other than first order.arrow_forwardMany biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.arrow_forward
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Kinetics: Initial Rates and Integrated Rate Laws; Author: Professor Dave Explains;https://www.youtube.com/watch?v=wYqQCojggyM;License: Standard YouTube License, CC-BY