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chemistry a molecular approach

Questions and Answers of Chemistry A Molecular Approach

Have each group member select and study a material from the section on ceramics, cement, and glass. Take turns describing your material to the group, and see if they can identify the type of material
Describe how a common object or toy (e.g., a train, building blocks, or beads on a string) could represent the structure of a polymer. Describe how the following terms would be represented using your
An alloy is a metallic mixture composed of two or more elements. As is the case in all mixtures, the relative amounts of the elements in an alloy can vary. In some cases, the components of an alloy
Consider the table listing the solubilities of several alcohols in water and in hexane. Which statement best describes the observed trend in terms of intermolecular forces?(a) As you move down the
Which statement is true?(a) Ideal gases mix because mixing decreases their potential energy.(b) Ideal gases mix because mixing increases their potential energy.(c) Ideal gases mix because mixing
This graph shows the concentration of the reactant A in the reaction A → B. Determine the average rate of the reaction between 0 and 10 seconds.a) 0.07 M/s b) 0.007 M/s c) 0.86 M/s d) 0.014 M/s
For the reaction A + 2B → C under a given set of conditions, the initial rate is 0.100 M/s. What is Δ[B]/Δt under the same conditions?(a) -0.0500 M/s(b) -0.100 M/s(c) -0.200 M/s(d) +0.200 M/s
Explain why lizards become sluggish in cold weather. How is this phenomenon related to chemistry?
Consider this balanced chemical equation:In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.(a) Calculate the average rate of this reaction in this time
For a particular reaction in which A → products, a doubling of the concentration of A causes the reaction rate to double. What is the order of the reaction?(a) 0 (b) 1 (c) 2
Dinitrogen monoxide decomposes into nitrogen and oxygen when heated. The initial rate of the reaction is 0.022 M/s.What is the initial rate of change of the concentration of N2O (that is,
Why are reaction rates important (both practically and theoretically)?
Consider the reaction between nitrogen dioxide and carbon monoxide:The initial rate of the reaction is measured at several different concentrations of the reactants, and the tabulated results are
The reaction A → B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of A of 0.100 M. What is the initial rate at [A] = 0.500 M ?(a)
This plot shows the rate of the decomposition of SO2Cl2 into SO2 and Cl2 as a function of the concentration of SO2Cl2.What is the order of the reaction?a) First order b) Second order c) Zero
Consider the equation for the decomposition of SO2Cl2:The concentration of SO2Cl2 is monitored at a fixed temperature as a function of time during the decomposition reaction, and the following data
What units are typically used to express the rate of a reaction?
This reaction was experimentally determined to be first order with respect to O2 and second order with respect to NO:The diagrams shown here represent reaction mixtures in which the number of each
For the reaction 2 A + B → C, the initial rate is measured at several different reactant concentrations. From the resulting tabulated data, determine the rate law for the reaction.a) Rate =
In Example 15.3, you determined that the decomposition of SO2Cl2 (under the given reaction conditions) is first order and has a rate constant of +2.90 * 10-4 s-1. If the reaction is carried out at
Why is the reaction rate for reactants defined as the negative of the change in reactant concentration with respect to time, whereas for products it is defined as the change in reactant concentration
The images shown here depict the first-order reaction A → B at various times during the reaction process. The black circles represent reactant A, and the red circles represent product B. What is
What is the rate constant for the reaction in Question 4?Question 4For the reaction 2 A + B → C, the initial rate is measured at several different reactant concentrations. From the resulting
Consider the equation for the decomposition of NO2:The concentration of NO2 is monitored at a fixed temperature as a function of time during the decomposition reaction and the data tabulated in the
Explain the difference between the average rate of reaction and the instantaneous rate of reaction.
The decomposition of Br2 is followed as a function of time; two different plots of the data are shown. Determine the order and rate constant for the reaction. In
Consider a simple reaction in which reactant A forms products:What is the rate law if the reaction is zero order with respect to A? First order? Second order? For each case, explain how a doubling of
A decomposition reaction, with a rate that is observed to slow down as the reaction proceeds, has a halflife that depends on the initial concentration of the reactant. Which statement is most likely
The reaction X → products is second order in X and has a rate constant of 0.035 M-1s-1. If a reaction mixture is initially 0.45 M in X, what is the concentration of X after 155 seconds?a) 7.6 Mb)
The decomposition of ozone shown here is important to many atmospheric reactions:A study of the kinetics of the reaction results in the following data:Determine the value of the frequency factor and
How is the order of a reaction generally determined?
Which statement best explains why reaction rates generally increase with increasing temperature?(a) Reaction rates increase with increasing temperature because, as temperature increases, a greater
A decomposition reaction has a half-life that does not depend on the initial concentration of the reactant. What is the order of the reaction?a) Zero order b) First order c) Second order d) Order
Consider the reaction between nitrogen dioxide and carbon monoxide:The rate constant at 701 K is measured as 2.57 M-1 · s-1 and that at 895 K is measured as 567 M-1 · s-1. Find the activation
For a reaction with multiple reactants, how is the overall order of the reaction defined?
A and reaction B have identical frequency factors. However, reaction B has a higher activation energy than reaction A. Which reaction has a greater rate constant at room temperature?(a) Reaction
The rate constant of a reaction is measured at different temperatures. A plot of the natural log of the rate constant as a function of the inverse of the temperature (in kelvins) yields a straight
Ozone naturally decomposes to oxygen by this reaction:The experimentally observed rate law for this reaction is:Show that this proposed mechanism is consistent with the experimentally observed rate
Explain the difference between the rate law for a reaction and the integrated rate law for a reaction. What relationship does each kind of rate law express?
Which reaction do you expect to have the smallest orientation factor? (a) H(g) + I(g) — HI(g) (b) H₂(g) + 12(g) → 2 HI(g) (c) HCl(g) + HCI(g) H₂(g) + Cl₂(8)
The rate constant for a reaction at 25.0 °C is 0.010 s-1, and its activation energy is 35.8 kJ. Find the rate constant at 50.0 °C.a) 0.021 s-1b) 0.010 s-1c) 0.0033 s-1d) 0.031 s-1
Write integrated rate laws for zero-order, first-order, and secondorder reactions of the form A → products.
The mechanism shown is proposed for the gas-phase reaction, 2 N2O5 → 4 NO2 + O2. What rate law does the mechanism predict?a) Rate = k[N2O5]b) Rate = k[N2O5]2c) Rate = k[N2O5]0d) Rate = k[NO2][NO3]
What is the rate law for the elementary step Cl + CO → ClCO ?(a) Rate = k[Cl] (b) Rate = k[CO](c) Rate = k[ClCO](d) Rate = k[Cl][CO]
What does the term half-life mean? Write the expressions for the half-lives of zero-order, first-order, and second-order reactions.
Which statement is true regarding the function of a catalyst in a chemical reaction?a) A catalyst increases the rate of a reaction.b) A catalyst provides an alternate mechanism for the reaction.c) A
How do reaction rates typically depend on temperature? What part of the rate law is temperature dependent?
These images represent the first-order reaction A → B initially and at some later time. The rate law for the reaction is Rate = 0.010 s-1 [A]. How much time has passed between the two images?a) 69
Explain the meaning of each term within the Arrhenius equation: activation energy, frequency factor, and exponential factor.Use these terms and the Arrhenius equation to explain why small changes in
Use collision theory to determine which single-step reaction has the smallest orientation factor.a) H + H → H2b) I + HI → I2 + Hc) H2 + H2C = CH2 → H3C—CH3d) All of these reactions have the
What is an Arrhenius plot? Explain the significance of the slope and intercept of an Arrhenius plot.
Carbon monoxide and chlorine gas react to form phosgene (COCl2) according to the equation:The rate law for the reaction is Rate = k[Cl2]3/2[CO]. Which representation of a mixture of chlorine gas and
Explain how a chemical reaction occurs according to the collision model. Explain the meaning of the orientation factor in this model.
Explain the difference between a normal chemical equation for a chemical reaction and the mechanism of that reaction.
In a reaction mechanism, what is an elementary step? Write down the three most common elementary steps and the corresponding rate law for each one.
What are the two requirements for a proposed mechanism to be valid for a given reaction?
What is a catalyst? How does a catalyst increase the rate of a chemical reaction?
What is an intermediate within a reaction mechanism?
Explain the difference between homogeneous catalysis and heterogeneous catalysis.
What are the four basic steps involved in heterogeneous catalysis?
What are enzymes? What is the active site of an enzyme? What is a substrate?
What is the general two-step mechanism by which most enzymes work?
Consider the reaction:2 N2O(g) → 2 N2(g) + O2(g)a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.b. In the first 15.0 s of the
For the reaction 2 A(g) + B(g) → 3 C( g),a. Determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.b. When A is
For the reaction A(g) + 1/2 B(g) → 2 C(g), a. Determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.b. When C is
Consider the reaction: Cl2(g) + 3 F2(g) → 2 ClF3(g)Complete the table. A[Cl₂]/At A[F₂]/At -0.012 M/s A[CIF3]/At Rate
Consider the reaction:8 H2S(g) + 4 O2(g) → 8 H2O(g) + S8(g)Complete the table. A[H₂S]/At A[0₂]/At -0.080 M/s A[H₂O]/At A[Ss]/At Rate
Consider the reaction:C4H8(g) → 2 C2H4(g)The tabulated data were collected for the concentration of C4H8 as a function of time:a. What is the average rate of the reaction between 0 and 10 s?
Consider the reaction:NO2(g) → NO(g) + 1/2 O2(g)The tabulated data were collected for the concentration of NO2 as a function of time:a. What is the average rate of the reaction between 10 and 20 s?
This graph shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A → products.a. What is the order of the reaction with respect to A?b. Make a rough
Consider the reaction:2 H2O2(aq) → 2 H2O(l) + O2(g)The graph shows the concentration of H2O2 as a function of time.Use the graph to calculate each quantity:a. The average rate of the reaction
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.a. What is the order of the reaction with respect to A?b. Make a rough sketch of a plot of [A] versus
What are the units of k for each type of reaction?a. First-order reactionb. Second-order reactionc. Zero-order reaction
This reaction is first order in N2O5:The rate constant for the reaction at a certain temperature is 0.053/s.a. Calculate the rate of the reaction when [N2O5] = 0.055 M.b. What would the rate of the
Consider the data showing the initial rate of a reaction (A → products) at several different concentrations of A.What is the order of the reaction? Write a rate law for the reaction, including the
Consider the data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction, including the
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.What is the order of the reaction? Write a rate law for the reaction,
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.What is the order of the reaction? Write a rate law for the reaction,
The tabulated data were collected for this reaction:Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction? 2
The tabulated data were collected for this reaction:Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?
Indicate the order of reaction consistent with each observation.a. A plot of the concentration of the reactant versus time yields a straight line.b. The reaction has a half-life that is independent
The tabulated data show the concentration of AB versus time for this reaction:Determine the order of the reaction and the value of the rate constant. Predict the concentration of AB at 25 s.
Indicate the order of reaction consistent with each observation.a. The half-life of the reaction gets shorter as the initial concentration is increased.b. A plot of the natural log of the
The tabulated data show the concentration of N2O5 versus time for this reaction:Determine the order of the reaction and the value of the rate constant. Predict the concentration of N2O5 at 250 s.
The tabulated data show the concentration of cyclobutane (C4H8) versus time for this reaction:Determine the order of the reaction and the value of the rate constant. What is the rate of reaction when
The reaction A → products was monitored as a function of time. The results are shown here.Determine the order of the reaction and the value of the rate constant. What is the rate of reaction when
This reaction was monitored as a function of time:A plot of ln[A] versus time yields a straight line with slope -0.0045/s.a. What is the value of the rate constant (k) for this reaction at this
This reaction was monitored as a function of time:A plot of 1/[AB] versus time yields a straight line with a slope of +0.55/M · s.a. What is the value of the rate constant (k) for this reaction at
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42 * 10-4s-1 at a certain temperature.a. What is the half-life for this reaction?b. How long will it take for the
The decomposition of XY is second order in XY and has a rate constant of 7.02 * 10-3M-1 · s-1 at a certain temperature.a. What is the half-life for this reaction at an initial concentration of 0.100
The half-life for the radioactive decay of U-238 is 4.5 billion years and is independent of initial concentration. How long will it take for 10% of the U-238 atoms in a sample of U-238 to decay? If a
The half-life for the radioactive decay of C-14 is 5730 years and is independent of the initial concentration. How long does it take for 25% of the C-14 atoms in a sample of C-14 to decay? If a
A chemical reaction is endothermic and has an activation energy that is twice the value of the enthalpy change of the reaction. Draw a diagram depicting the energy of the reaction as it progresses.
H2 and I2 are combined in a flask and allowed to react according to the reaction:Examine the figures (sequential in time) and answer the questions:a. Which figure represents the point at which
Calculate the pH of a buffer solution that is 0.050 M in benzoic acid (HC7H5O2) and 0.150 M in sodium benzoate (NaC7H5O2). For benzoic acid, Ka = 6.5 * 10-5.
Closely examine Figure 18.3. Which image best represents the amount of OH- added to the buffer in part (b) of the figure? a. b. C.
The activation energy of a reaction is 56.8 kJ/mol, and the frequency factor is 1.5 * 1011/s. Calculate the rate constant of the reaction at 25 °C.
The rate constant of a reaction at 32 °C is 0.055/s. If the frequency factor is 1.2 * 1013/s, what is the activation barrier?
The rate constant (k) for a reaction was measured as a function of temperature. A plot of ln k versus 1/T (in K) is linear and has a slope of -7445 K. Calculate the activation energy for the reaction.
The data shown here were collected for the first-order reaction:Use an Arrhenius plot to determine the activation barrier and frequency factor for the reaction. N₂O(g) N₂(g) + O(g)

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