Chemistry: Structure and Properties (2nd Edition)
2nd Edition
ISBN: 9780134293936
Author: Nivaldo J. Tro
Publisher: PEARSON
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Chapter 14, Problem 116E
Interpretation Introduction
To determine: The length of time for each system to reach a specified total pressure and the total pressure after a specific period of time.
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Chapter 14 Solutions
Chemistry: Structure and Properties (2nd Edition)
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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- Hydrogen peroxide, H2O2(aq), decomposes to H2O() and O2(g) in a reaction that is first-order in H2O2 and has a rate constant k = 1.06 103 min1 at a given temperature. (a) How long will it take for 15% of a sample of H2O2 to decompose? (b) How long will it take for 85% of the sample to decompose?arrow_forwardThe following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.arrow_forwardAn excellent way to make highly pure nickel metal for use in specialized steel alloys is to decompose Ni(CO)4 by heating it in a vacuum to slightly above room temperature. Ni(CO)4(g) Ni(s) + 4 CO(g) The reaction is proposed to occur in four steps, the first of which is Ni(CO)4(g) Ni(CO)3(g) + CO(g) Kinetic studies of this first-order decomposition reaction have been carried out between 47.3 C and 66.0 C to give the results in the table. (a) Determine the activation energy for this reaction. (b) Ni(CO)4 is formed by the reaction of nickel metal with carbon monoxide. Suppose that 2.05 g CO is combined with 0.125 g nickel metal. Determine the maximum mass (g) of Ni(CO)4 that can be formed. Replacement of CO by another molecule in Ni(CO)4 was studied in the nonaqueous solvents toluene and hexane to understand the general principles that govern the chemistry of such compounds. Ni(CO)4(g) + P(CH3)3 Ni(CO)3P(CH3)3 + CO A detailed study of the kinetics of the reaction led to the mechanism Step1:(slow)Ni(CO)4Ni(CO)3+COStep2:(fast)Ni(CO)3+P(CH3)3Ni(CO)3P(CH3)3 (c) Which step in the mechanism is unimolecular? Which is bimolecular? (d) Add the steps of the mechanism to show that the result is the balanced equation for the observed reaction. (e) Is there an intermediate in this reaction? If so, what is it? (f) It was found that doubling the concentration of Ni(CO)4 increased the reaction rate by a factor of 2. Doubling the concentration of P(CH3)3 had no effect on the reaction rate. Based on this information, write the rate equation for the reaction. (g) Does the experimental rate equation support the proposed mechanism? Why or why not?arrow_forward
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