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Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

Using Figures 9.35 and 9.43 as guides, draw the molecular orbital electron configuration for(a) B2+(b) Li2+(c) N2+(d) Ne22+In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species.
If we assume that the energy-level diagrams for homo nuclear diatomic molecules shown in Figure 9.43 can be applied to hetero nuclear diatomic molecules and ions, predict the bond order and magnetic behavior of(a) CO+(b) NO-(c) OF+(d) NeF+
Determine the electron configurations for CN+, CN, and CN-.(a) Which species has the strongest C-N bond?(b) Which species, if any, has unpaired electrons?
(a) The nitric oxide molecule, NO, readily loses one electron to form the NO+ ions. Why is this consistent with the electronic structure of NO? (b) Predict the order of the N-O bond strengths in NO, NO+, and NO-, and describe the magnetic properties of each. (c) With what neutral homo nuclear
Consider the molecular orbitals of the P2 molecule. Assume that the MOs of di-atomics from the third row of the periodic table are analogous to those from the second row.(a) Which valence atomic orbitals of P are used to construct the MOs of P2?(b) The figure that follows shows a sketch of one of
The iodine bromide molecule, IBr, is an inter-halogen compound. Assume that the molecular orbitals of IBr are analogous to the homo nuclear diatomic molecule F2.(a) Which valence atomic orbitals of I and of Br are used to construct the MOs of IBr?(b) What is the bond order of the IBr molecule?(c)
(a) What is the physical basis for the VSEPR model? (b) When applying the VSEPR model, we count a double or triple bond as a single electron domain. Why is this justified?
What is the fundamental basis on which we assign electrons to electron domains in pairs and with their spins paired?
The molecules SiF4, SF4, and XeF4 have molecular formulas of the type AF4, but the molecules have different molecular geometries. Predict the shape of each molecule, and explain why the shapes differ.
For each of these contour representations of molecular orbitals, identify(a) The atomic orbitals (s or p) used to construct the MO(b) The type of MO (or),(c) Whether the MO is bonding or anti-bonding,(d) The locations of nodal planes.
Consider the molecule PF4Cl. (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry. (b) Which would you expect to take up more space, a P-F bond or a P-Cl bond? Explain. (c) Predict the molecular geometry of PF4Cl.How did your answer for part (b) influence your
The vertices of a tetrahedron correspond to four alternating corners of a cube. By using analytical geometry, demonstrate that the angle made by connecting two of the vertices to a point at the center of the cube is 109.5o, the characteristic angle for tetrahedral molecules.
From their Lewis structures, determine the number of σ and π bonds in each of the following molecules or ions: (a) CO2 (b) Cyanogen, (CN)2; (c) Formaldehyde, H2CO (d) Formic acid, HCOOH, which has one H and two O atoms attached to C.
The lactic acid molecule, CH3CH (OH) COOH, gives sour milk its unpleasant, sour taste. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many π and how many σ bonds are in the molecule? (c) Which CO bond is shortest in
The PF3 molecule has a dipole moment of 1.03 D, but BF3 has a dipole moment of zero. How can you explain the difference?
An AB5 molecule adopts the geometry shown here.(a) What is the name of this geometry?(b) Do you think there are any nonbonding electron pairs on atom A? Why or why not?(c) Suppose the atoms B are halogen atoms. Can you determine uniquely to which group in the periodic table atom A belongs?
There are two compounds of the formula Pt(NH3)2Cl2:The compound on the right, cisplatin, is used in cancer therapy. The compound on the left, transplatin, is ineffective for cancer therapy. Both compounds have a square-planar geometry. (a) Which compound has a nonzero dipole moment? (b) The reason
The O-H bond lengths in the water molecule (H2O) are 0.96 Ã…, and the H-O-H angle is 104.5º. The dipole moment of the water molecule is 1.85 D.(a) In what directions do the bond dipoles of the O-H bonds point? In what direction does the dipole moment vector of the water molecule
The reaction of three molecules of fluorine gas with a Xe atom produces the substance xenon hexafluoride, XeF6:Xe(g) + 3 F2(g) → XeF6(s)(a) Draw a Lewis structure for XeF6.(b) If you try to use the VSEPR model to predict the molecular geometry of XeF6, you run into a problem. What is it?(c) What
The Lewis structure for allene isMake a sketch of the structure of this molecule that is analogous to Figure 9.25. In addition, answer the following three questions: (a) Is the molecule planar? (b) Does it have a nonzero dipole moment? (c) Would the bonding in allene be described as delocalized?
For which one of the following vessels for the reaction A + B ---†’ C is the reaction the fastest? Assume all vessels are at the same temperature.
You study the effect of temperature on the rate of two reactions and graph the natural logarithm of the rate constant for each reaction as a function of 1/T. How do the two graphs compare: (a) If the activation energy of the second reaction is higher than the activation energy of the first reaction
Consider the following reaction between mercury (II) chloride and oxalate ion:2 HgCI2(aq) + C2O42- (aq) †’2 CIË‰ (aq) + 2 CO2(g) + Hg2CI2(s)The initial rate of this reaction was determined for several concentration of HgCI2 and C2O42-, and the following rate data were obtained
The reaction 2 NO2 → 2 NO + O2 has the rate constant. k = 0.63 M-1s-1. Based on the units for k, is the reaction first or second order in NO2? If the initial concentration of NO2 is 0.100M, how would you determine how long it would take for the concentration to decrease to 0.025 M?
Consider two reactions. Reaction (1) has a constant half-life, whereas reaction (2) has a half-life that gets longer as the reaction proceeds. What can you conclude about the rate laws of these reactions from these observations?
When chemists are performing kinetics experiments, the general rule of thumb is to allow the reaction to proceed for 4 half-lives. (a) Explain how you would be able to tell that the reaction has proceeded for 4 half-lives. (b) Let us suppose a reaction A → B takes 6 days to proceed for 4
(a) The reaction is first H2O2(aq) → H2O(I) + ½ O2(g) is first order. Near room temperature, the rate constant equals 7.0 × 10-4s-1. Calculate the half-life at this temperature. (b) At 415 oC, (CH2)2O decomposes in the gas phase, (CH2)2O(g) → CH4(g) + CO(g). If the reaction is first order
Americium-241 is used in smoke detectors. It has a first order rate constant for radioactive decay of k = 1.6 × 10-3 yr -1. By contrast, iodine-125, which is used to test for thyroid functioning, has a rate constant for radioactive decay of k = 0.011 day-1. (a) What are the half-lives of these two
Urea (NH2CONH2) is the end product in protein metabolism in animals. The decomposition of urea in 0.1 M HCl occurs according to the reaction NH2CONH2 (aq) + H+ (aq) + 2 H2O(I) → 2 NH4+ (aq) + HCO3 ˉ(aq) The reaction is first order in urea and first order overall. When [NH2CONH2] = 0.200 M,
The rate of a first-order reaction is followed by spectroscopy, monitoring the absorbance of a colored reactant at 520 nm. The reaction occurs in a 1.00-cm sample cell, and the only colored species in the reaction has an extinction coefficient of 5.60 × 103 M-1 cm-1 at 520 nm. (a) Calculate the
A colored dye compound decomposes to give a colorless product. The original dye absorbs at 608 nm and has an extinction coefficient of 4.7 × 104 M-1 cm-1 at that wavelength. You perform the decomposition reaction in a 1-cm cuvette in a spectrometer and obtain the following data: Time
Cyclopentadiene (C5H6) reacts with itself to form dicyclopentadiene (C10H12). A 0.0400 M solution of C5H6 was monitored as a function of time as the reaction 2 C5H6 → C10H12 proceeded. The following data were collected: Time (s) [C5H6]
The following graph shows two different reaction pathways for the same overall reaction at the same temperature.(a) Which pathway is slower? Why?(b) How can there be two different reaction pathways for the same reaction at the same temperature? Discuss.
(a) Two reactions have identical values for Ea. Does this ensure that they will have the same rate constant if run at the same temperature? Explain. (b) Two similar reactions have the same rate constant at 25 oC, but at 35 oC one of the reactions has a larger rate constant than the other. Account
The first order rate constant for reaction of a particular organic compounded with water varies with temperature as follows: Temperature (K) Rate Constant (s-1) 300................................3.2 × 10-11 320................................1.0 × 10-9 340................................3.0 ×
The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O: NO(g) + NO(g) → N2O2(g)N2O2 + H2(g) → N2O(g) + H2O(g)(a) Show that the elementary reactions of the proposed mechanism add to provide a balanced equation for the reaction.(b) Write a rate law for each
Ozone in the upper atmoshphere can be destroyed by the following two step mechanism:Cl(g) + O3(g) → ClO(g) + O2(g)Cl(g) + O(g) → ClO(g) + O2(g)(a)What is the overall equation for this process? (b) What is the catalyst in the reaction? How do you know?(c) What is the intermediate in the
Using Figure 14.23 as your basis, draw the energy profile for the bromide-catalyzed decomposition of hydrogen peroxide. (a) Label the curve with the activation energies for reactions [14.30] and [14.31].
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine:Step 1:Step 2:Step 3:(a) What is the overall reaction?(b) What are the intermediates in the mechanism?(c) What is the molecularity of each of the elementary reactions?(d) What is the
In a hydrocarbon solution, the gold compound (CH3)3AuPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AuPH3. The following mechanism has been proposed for the decomposition of (CH3)3AuPH3: Step 1: (fast) Step 2: (slow) Step 3: (fast) (a) What is the overall reaction? (b)
Enzymes are often described as following the two-step mechanism:ES --†’ E + P (slow)Where E = enzyme, S = substrate, ES = enzyme - substrate complex, and P = product.(a) If an enzyme follows this mechanism, what rate law is expected for the reaction?(b) Molecules that can bind to the active
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45oC of 1.0 × 10-5 s-1. Calculate the partial pressure of O2 produced from 1.00 L of 0.600 M N2O5 solution at over a period of 20.0 hr if the gas is
Consider the diagram that follows, which represents two steps in an overall reaction. The red spheres are oxygen, the blue ones nitrogen, and the green ones fluorine.(a) Write the chemical equation for each step in the reaction.(b) Write the equation for the overall reaction.(c) Identify the
The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OHˉ (alc) --→ C2H5OH(I) + Iˉ(alc), has an activation energy of and a frequency factor of 2.10 × 1011 M-1 s-1. (a) Predict the rate constant for the reaction at 35 oC. (b) A solution of KOH in ethanol
You obtain kinetic data for a reaction at a set of different temperatures. You plot ln k versus 1/T and obtain the following graph:Suggest a molecular-level interpretation of these unusual data.
The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kJ/mol and a frequency factor of A = 6.0 × 108 M-1s-1. The reaction is believed to be bimolecular:(a) Calculate the rate constant at 100 oC.(b) Draw the Lewis structures for the NO and the NOF molecules,
The mechanism for the oxidation of HBr by O2 to form 2 H2O and Br2 is shown in Exercise 14.80.(a) Calculate the overall standard enthalpy change for the reaction process.(b) HBr does not react with O2 at a measurable rate at room temperature under ordinary conditions. What can you infer from this
The rates of many atmospheric reactions are accelerated by the absorption of light by one of the reactants. For example, consider the reaction between methane and chlorine to produce methyl chloride and hydrogen chloride:Reaction 1: CH4(g) + CI2(g) †’ CH3CI(g) + HCI(g)This reaction is
Many primary amines, RNH2, where R is a carbon containing fragment such as CH3, CH3CH2, and so on, undergo reactions where the transition state is tetrahedral. (a) Draw a hybrid orbital picture to visualize the bonding at the nitrogen in a primary amine (just use a C atom for "R"). (b) What kind of
The NOx waste stream from automobile exhaust includes species such as NO and NO2. Catalysts that convert these species to N2 are desirable to reduce air pollution. (a) Draw the Lewis dot and VSEPR structures of NO, NO2, and N2. (b) Using a resource such as Table 8.4, look up the energies of the
Based on the following reaction profile, how many intermediates are formed in the reaction A --†’ C? How many transition states are there? Which step is the fastest? Is the reaction A --†’ C exothermic or endothermic?
Draw a possible transition state for the bimolecular reaction depicted here. (The blue spheres are nitrogen atoms, and the red ones are oxygen atoms.) Use dashed lines to represent the bonds that are in the process of being broken or made in the transition state?
The following diagram represents an imaginary two-step mechanism. Let the red spheres represent element A, the green ones element B, and the blue ones element C.(a) Write the equation for the net reaction that is occurring.(b) Identify the intermediate.(c) Identify the catalyst.
Draw a graph showing the reaction pathway for an overall exothermic reaction with two intermediates that are produced at different rates. On your graph indicate the reactants, products, intermediates, transition states, and activation energies?
(a) What is meant by the term reaction rate? (b) Name three factors that can affect the rate of a chemical reaction? (c) Is the rate of disappearance of reactants always the same as the rate of appearance of products? Explain.
(a)What are the units usually used to express the rates of reactions occurring in solution? (b) From your everyday experience, give two examples of the effects of temperature on the rates of reactions? (c) What is the difference between average rate and instantaneous rate?
Consider the following hypothetical aqueous reaction:A (aq) --†’ flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected:(a) Calculate the number of moles of B at each time in the table, assuming that there are no molecules of B at time zero,
Consider the following graph of the concentration of a substance over time.(a) Is X a reactant or product of the reaction?(b) Is the reaction speeding up, slowing down, or not changing its rate as time progresses?(c) Why is the average rate of the reaction different between points 1 and 2 than
A flask is charged with 0.100 mol of A and allowed to react to from B according to the hypothetical gas-phase reaction A(g) --†’ B(g). The following are collected:(a) Calculate the number of moles of B at each time in the table, assuming that A is cleanly converted to B with no
The isomerization of methyl isonitrile (CH3NC) to acetonitrile (CH3CN) was studied in the gas phase at 215 oC, and the following data were obtained: Time (s) [CH3NC] (M) 0..........................0.0165 2, 000....................0.0110 5, 000....................0.00591 8,
The rate of disappearance of HCl was measured for the following reaction: CH3OH(aq) + HCI(aq) --→ CH3CI(aq) + H2O(I) The following data were collected: Time (min) [HCI]
For each of the following gas-sphase reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance of each product: (a) H2O2(g) --→ H2(g) + O2(g) (b) 2 N2O(g) --→ 2 N2(g) + O2(g) (c) N2(g) + 3 H2(g) --→ 2 NH3(g) (d) C2H5NH2(g) --→ C2H4(g) + NH3(g)?
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) --→
(a) Consider the combustion of H2(g): 2 H2(g) + O2(g) --→ 2 H2O(g), 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? (b) The reaction 2 NO(g) + CI2(g) --→ 2 NOCI(g) is carried out in a closed vessel. If
(a) Consider the combustion of ethylene, C2H4(g) + 3 O2(g) --→ 2 CO2(g) + 2 H2O(g). If the concentration of C2H4 is decreasing at the rate of 0.036 M/s, what are the rates of change in the concentrations of CO2 and H2O? (b) The rate of decrease in N2H4 partial pressure in a closed reaction vessel
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? Explain. (b) What are the reaction orders for A and B? What is the overall reaction order? (c) What are the units of the rate constant?
Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (a) Write the rate law for the reaction. (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
The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 --→ 4 NO2 + O2. The rate law is first order in N2O5. At the rate constant is 4.82 × 10-3 s-1. (a) Write the rate law for the reaction. (b) What is the rate of reaction when [N2O5] = 0.0240 M? (c) What happens to the rate when
You study the rate of a reaction, measuring both the concentration of the reactant and the concentration of the product as a function of time, and obtain the following results:Which chemical equation is consistent with these data: (a) A ----†’ B, (b) B ----†’ A, (c) A
Consider the following reaction: 2 NO(g) + 2 H2(g) --→ N2(g) + 2 H2O(g) (a) The rate law for this reaction is first order in H2 and second order in NO. Write the rate law. (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
Consider the following reaction: CH3Br(aq) + OHˉ (aq) --→ CH3OH(aq) + Brˉ(aq) The rate law for this reaction is first order in CH3Br and first order in OHˉ. When [CH3Br] is 5.0 × 10-3 M and [OHˉ] 0.050 M, the reaction rate at 298 K is 0.0432 M/s. (a) What is the value of the rate
The reaction between ethyl bromide (C2H5Br) and hydroxide ion in ethyl alcohol at 330 K, C2H5Br(alc) + OHˉ (alc) --→ C2H5OH(I) + Brˉ(aIc), is first order each in ethyl bromide and hydroxide ion. When [C2H5Br] is 0.0477 M and [OHˉ] is 0.100 M, the rate of disappearance of ethyl bromide is 1.7
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCI + IË‰ --†’ OIË‰ + CIË‰. This rapid reaction gives the following rate data:(a) Write the rate law for this reaction. (b) Calculate the rate
The reaction 2 CIO2(aq) + 2 OHË‰(aq) --†’ CIO3Ë‰ (aq) + CIO2Ë‰(aq) + H2O(I) was studied with the following results:(a) Determine the rate law for the reaction (b) Calculate the rate constant with proper units. (c) Calculate the rate when [CIO2] = 0.100 M and
The following data where measured for the reaction BF3(g) + NH3(g) --†’ F3BNH3(g):(a) What is the rate law for the reaction? (b)What is the overall order of the reaction? (c) Calculate the rate constant with proper units? (d) What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M?
The following data were collected for the rate of disappearance of NO in the reaction 2 NO(g) + O2(g) --†’ 2 NO2(g):(a) What is the rate law for the reaction? (b) What are the units of the rate constant? (c) What is the average value of the rate constant calculated from the three data
Consider the gas-phase reaction between nitric oxide and bromine at 273 oC: 2 NO(g) + Br2(g) †’ 2. The following data for the initial rate of appearance of NOBr were obtained:(a) Determine the rate law. (b) Calculate the average value of the rate constant for the appearance of NOBr from
Consider the reaction of peroxydisulfate ion (S2O8-2) with iodide ion (Iˉ) in aqueous solution: S2O82- (aq) + 3 Iˉ (aq) -→ 2 SO42- (aq) + I3ˉ(aq) At a particular temperature the initial rate of disappearance S2O82- of varies with reactant concentrations in the following manner: (a) Determine
(a) Define the following symbols that are encountered in rate equations for the generic reaction A → B: [A]0, t1/2 [A]t, k. (b) What quantity, when graphed versus time, will yield a straight line for a first-order reaction? (c) How can you calculate the rate constant for a first-order reaction
You perform the reaction K + L †’ M, monitor the production of M over time, and then plot this graph from your data:(a) Is the reaction occurring at a constant rate from t = 0 to t = 15 min? Explain. (b) Is the reaction completed at t = 15 min? Explain.
(a) For a generic second-order reaction A → B, what quantity, when graphed versus time, will yield a straight line? (b) What is the slope of the straight line from part (a)? (c) How do the half-lives of first-order and second-order reactions differ?
For the generic reaction A → B that is zero order in A, what would you graph in order to obtain the rate constant?
Sketch a graph for the generic first-order reaction A → B that has concentration of A on the vertical axis and time on the horizontal axis. (a) Is this graph linear? Explain. (b) Indicate on your graph the half-life for the reaction?
(a) The gas-phase decomposition of SO2Cl2, SO2Cl2(g) → SO2(g) + CI2(g), is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 × 105 s. What is the rate constant at this temperature? (b) At 320 oC the rate constant is 2.2 × 10-5s-1. What is the half-life at this temperature?
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 sˉ. (a) What is the half-life for this reaction? (b) If you start with 0.050 M I2 at this temperature, how much will remain after 5.12 s assuming that the iodine atoms do not recombine to form
As described in Exercise 14.43, the decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 × 10-2s-1. (a) If we begin with an initial SO2Cl2 pressure of 450 torr, what is the pressure of this substance after 60 s? (b) At what
The first-order rate constant for the decomposition of N2O5, 2 N2O5(g) → 4 NO2(g) + O2(g), at is 70 oC is 6.82 × 10-3 s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 2.0 L. (a) How many moles of N2O5 will remain after 5.0 min? (b) How many minutes will it take for the quantity of
The reaction SO2CI2(g) → SO2(g) + CI2(g) is first order in SO2Cl2.Using the following kinetic data, determine the magnitude and units of the first-order rate constant: Time (s) Pressure SO2CI2 (atm) 0..........................1.000 2, 500....................0.947 5,
From the following data for the first-order gas-phase isomerization of CH3NC at 215 oC, calculate the first-order rate constant and half-life for the reaction: Time (s) Pressure CH3NC (torr) 0..........................502 2, 000....................335 5, 000....................180 8,
Consider the data presented in Exercise 14.19. (a) By using appropriate graphs, determine whether the reaction is first order or second order. (b) What is the rate constant for the reaction? (c) What is the half-life for the reaction?
You perform a series of experiments for the reaction A --→ B + C and find that the rate law has the form. Rate = k[A]x. Determine the value of x in each of the following cases: (a) There is no rate change when is tripled. (b) The rate increases by a factor of 9 when is tripled. (c) When is
Consider the data presented in Exercise 14.20. (a) Determine whether the reaction is first order or second order. (b) What is the rate constant? (c) What is the half-life?
The gas-phase decomposition of NO2, 2 NO2(g) → 2 NO(g) + O2(g), is studied at 383 oC, giving the following data: Time (s) [NO2]
Sucrose (C12H22O11), commonly known as table sugar, reacts in dilute acid solutions to form two simpler sugars, glucose and fructose, both of which have the formula C6H12O6. At 23 oC and in 0.5 M HCl, the following data were obtained for the disappearance of sucrose: Time (min) [C12H22O11]
(a) What factors determine whether a collision between two molecules will lead to a chemical reaction? (b) According to the collision model, why does temperature affect the value of the rate constant? (c) Does the rate constant for a reaction generally increase or decrease with an increase in
(a) In which of the following reactions would you expect the orientation factor to be least important in leading to reaction: NO + O → NO2 or H + CI → HCI? (b) How does the kinetic-molecular theory help us understand the temperature dependence of chemical reactions?
Calculate the fraction of atoms in a sample of argon gas at 400 K that has an energy of 10.0 kJ or greater?
(a) The activation energy for the isomerization of methyl isonitrile (Figure 14.7) is 160 kJ/mol. Calculate the fraction of methyl isonitrile molecules that has an energy of 160.0 kJ or greater at 500 K. (b) Calculate this fraction for a temperature of 520 K. What is the ratio of the fraction at
The gas-phase reaction CI(g) + HBr(g) → HCI(g) + Br(g) has an overall enthalpy change of - 66 kJ. The activation energy for the reaction is 7 kJ. (a) Sketch the energy profile for the reaction, and label Ea and (E. (b) What is the activation energy for the reverse reaction?
For the elementary process N2O5(g) → NO2(g) + NO3(g) the activation energy (Ea) and overall (E are 154 kJ/mol and 136 kJ/mol, respectively. (a) Sketch the energy profile for this reaction, and label Ea and (E. (b) What is the activation energy for the reverse reaction?

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