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engineering
chemical engineering

Questions and Answers of Chemical Engineering

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
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
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,
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
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
(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
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?
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
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
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
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
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
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
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
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)
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
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
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
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
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
(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,
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,
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) +
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
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
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
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
(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
The first order rate constant for reaction of a particular organic compounded with water varies with temperature as follows: Temperature (K) Rate Constant
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
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?
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
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
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
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
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
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
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 ×
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)
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
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
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
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
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
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
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
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,
(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
(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
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
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
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
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]
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
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)
(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
(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
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
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]
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
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
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
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
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.
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCI + IË‰ --†’ OIË‰ + CIË‰. This rapid reaction
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
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
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
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
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
(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
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
(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
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
(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
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
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
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
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
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
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
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
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
(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
(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
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
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
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

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