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(a)
Interpretation: The overall equation has to be given.
Concept introduction:
Molecularity: Elementary steps of a
Rate equations for elementary steps: The rate equation for elementary step is defined by its reaction stoichiometry.
(a)
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Answer to Problem 2CYU
The overall reaction is:
Explanation of Solution
The overall reaction is given as,
The overall reaction is:
(b)
Interpretation: The rate determining step has to be given.
Concept introduction:
The
The raise in molar concentration of product of a reaction per unit time or decrease in molarity of reactant per unit time is called rate of reaction and is expressed in units of
The variation in concentration of reaction or product over a certain interval of time is called average reaction rate.
The equation that relates the reaction rate to the reactants concentrations that is raised to various powers is called as rate law.
Rate law can be determined by the slow step or otherwise called as rate-determining step.
(b)
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Answer to Problem 2CYU
Step 2 is the rate determining step.
Explanation of Solution
The overall reaction is given as,
The rate determining step:
The rate of overall reaction is controlled by the slowest step in the mechanism. So, the step 2 is the slowest step which determines the rate of overall reaction.
(c)
Interpretation: The rate equation for the rate determining step has to be given.
Concept introduction:
The rate of reaction is the quantity of formation of product or the quantity of reactant used per unit time. The rate of reaction doesn’t depend on the sum of amount of reaction mixture used.
The raise in molar concentration of product of a reaction per unit time or decrease in molarity of reactant per unit time is called rate of reaction and is expressed in units of
The variation in concentration of reaction or product over a certain interval of time is called average reaction rate.
The equation that relates the reaction rate to the reactants concentrations that is raised to various powers is called as rate law.
Rate law can be determined by the slow step or otherwise called as rate-determining step.
(c)
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Explanation of Solution
Rate equation for rate-determining step:
The overall reaction is given as,
The rate determining step:
The rate of overall reaction is controlled by the slowest step in the mechanism. So, the step 2 is the slowest step which determines the rate of overall reaction.
The rate equation for the rate determining step is
(d)
Interpretation: The reaction intermediates has to be given.
(d)
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Answer to Problem 2CYU
The reaction intermediates are
Explanation of Solution
Intermediates are the molecules that are formed from the reactants and reacts to give the products in a chemical reaction. Hence, the two molecules that are generated in between the reaction and get turned to products are
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Chapter 14 Solutions
Chemistry & Chemical Reactivity
- The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardThe label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardThe hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?arrow_forward
- 1. (a) Show that decomposition of the organic compound 1,3-pentadiene is a second-order reaction and determine the rate constant. The concentration of 1,3-pentadiene was measured as a function of time. The data are as follows: (b) What is the value of the rate constant for the decomposition of 1,3-pentadiene.(c) What is the initial concentration for the reaction? Report to 3 significant figures.(d) What is the concentration of 1,3-pentadiene after 3.750 x10^3 s? Time(s) [1,3-pentadiene] (M) 0 .480 1000 .179 2000 .110 3000 .0795 4000 .0622 5000 .0510arrow_forwardIndicate whether each statement is true or false. (a) If you compare two reactions with similar collision factors, the one with the larger activation energy will be faster. (b) A reaction that has a small rate constant must have a small frequency factor. (c) Increasing the reaction temperature increases the fraction of successful collisions between reactants.arrow_forward2. (a) You study the effect of temperature on the rate of two reactions and graph the natural logarithm (In) of the rate constant for each reaction as a function of Explain, with the aid of diagrams and equations, how the two graphs compare if (i) The activation energy of the second reaction is higher than the activation energy of the first reaction but the two reactions have the same frequency factor. (ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction but the two reactions have the same activation energy.arrow_forward
- The reaction 2 ClO2(aq) + 2 OH- (aq)--->ClO3- (aq) +ClO2- (aq) + H2o(l) was studied with the followingresults: (a) Determine the rate law for the reaction. (b) Calculatethe rate constant with proper units. (c) Calculate the ratewhen [ClO2] = 0.100 M and [OH- ] = 0.050 M.arrow_forward3) In the first order "A Product" reaction at 25°C, the initial concentration of compound "A" is 0.8158 M, and its concentration after 15.9 minutes is 0.6311 M. For this first-order reaction, (a) What is the rate constant k, in min? (b) What is the half-life, in min? (c) What will be the molar concentration of "A" after 150 minutes? (d) If the activation energy of this reaction is 34.5 kJ/mol, at what temperature would the half- life of this reaction be 10.0 minutes?arrow_forwardAcetone is one of the most important solvents in organicchemistry, used to dissolve everything from fats and waxes toairplane glue and nail polish. At high temperatures, it decom-poses in a first-order process to methane and ketene(CH2=C=O). At 600C, the rate constant is 8.7x10^-3s⁻¹.(a) What is the half-life of the reaction?(b) How long does it take for 40.% of a sample of acetone todecompose?(c) How long does it take for 90.% of a sample of acetone todecompose?arrow_forward
- 5*) a) 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]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)arrow_forwardHydrogen peroxide, H2O2 (aq) decomposes to H2O (l) and O2 (g) in a reaction that is first order in H2O2 and has rate constantk = 1.06 × 10-3min-1.(i) How long will it take for 15% of a sample of H2O2 to decompose?(ii) How long will it take for 85% of the sample to decompose?arrow_forward1. Which of the following statements is incorrect? (A) The reaction in which the rate equation corresponds to a stoichiometric equation is called an elementary reaction. (B) Molecularity of a reaction may not be equal to the order of reaction. (C) With increase in temperature, the rate constant obeying Arrhenius equation decreases. (D) Rate of a chemical reaction is independent of the concentration of the reactants for a zero order reaction. 2. The rate of a gas phase reaction is given by, kCACB. If the volume of the reaction vessel is reduced to l/3rd of its initial volume, then the reaction rate compared to the original rate will be _____ times. (A) 3 (C) 6 (B) 9 (D) 12 3. A given number of molecules (i.e., moles) of a particular chemical species have reacted or disappeared when any of the following occurs except (A) Combination (C) Isomerization (B) Decomposition (D) Isolation Please Answer all!arrow_forward
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