(a)
Interpretation:
The initial rate at which the methyl acetate is converted to products when both reactants,
Concept Introduction:
The relationship between rate and initial concentration of reactant is described by rate law. It is an experimentally determined equation and cannot be found out theoretically from the stoichiometry of the reactants and products.
Where, ,
(b)
Interpretation:
The rate at which methyl alcohol
Concept Introduction:
Consider the following reaction.
Where
Where,
Rate of the reaction can be expressed in terms of change in concentration of reactant and products by multiplying the reciprocal of the corresponding stoichiometric co-efficient to that.
Want to see the full answer?
Check out a sample textbook solutionChapter 11 Solutions
Chemistry: The Molecular Science
- . Account for the increase in reaction rate brought about by a catalyst.arrow_forwardThe 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_forwardConsider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.arrow_forward
- Give at least two physical properties that might be used to determine the rate of a reaction.arrow_forwardWhich reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?arrow_forwardConsider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/sarrow_forward
- Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first order in H2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 79200, what is the reaction rate when [NO(g)] = 0.0852 M and [H2(g)] = 0.137 M?Rate =____ M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.170 M while the concentration of H2(g) is 0.137 M?Rate = ____ M/sarrow_forward7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?arrow_forwardWrite the reaction rate expressions for the following reactions in terms of the disappearance of the reactants and the appearance of products: (a) 2H2(g) + O2(g) -> 2H2O(g) (b) 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2(O)garrow_forward
- 4. The first order rate constant for the composition of chloroethane, C2HSCI(g) → C2H«(g) + HCI(g) at 700 K is 2.5 x 103 min1. Calculate: (a) (b) The half-life of chloroethane at 700 K. The concentration of chloroethane that remains after 60 min if the initial concentration is 0.10 M.arrow_forwardThe decomposition reaction on N2O5 in carbon tetrachloride is 2 N2 O5-----> 4NO2 + O2. The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 X 10-3s-1 (a) write the rate law for the reaction. (b) what is the rate when the concentration of N2O5 is doubled from 0.0240 M to 0.0480 M? Group of answer choices A) (a) rate= k[N2O5] (b) the rate doubles to 1.16 x 10E(-4) M/sec B.) (a) rate= k[N2O5] (b) the rate is halved to 5.8 x 10E(-5) M/sec C.) (a) rate= k[N2O5] (b) the rate doubles to 2.32 x 10E(-4) M/sec D.) (a) rate= k[N2O5]0 (b) the rate stays the samearrow_forwardConsider the reaction A + B ¡ C + D. Is each of the following statements true or false? (a) The rate law for the reaction must be Rate = k3A43B4. (b) If the reaction is an elementary reaction, the rate law is second order. (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order. (d) The activation energy for the reverse reaction must be greater than that for the forward reaction.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning