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(a)
Interpretation:
The order for the given reaction should be determined using the given set of data.
Concept introduction:
Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.
Rate constant: The rate constant for a
Rate order: The order of each reactant in a reaction is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.
(b)
Interpretation:
The rate constant for the given reaction should be determined using the given set of data.
Concept introduction:
Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.
Rate constant: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.
Rate order: The order of each reactant in a reaction is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.
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Chapter 14 Solutions
Chemistry & Chemical Reactivity
- Three first-order reactions have the following activation energies: (a) Which reaction is the fastest? (b) Which reaction has the largest half-life? (c) Which reaction has the largest rate?arrow_forward1. Which of the following statements is incorrect? (A) As the chemical reaction proceeds, the rate of reaction increases. (B) The reaction rate almost gets doubled for 10°C rise in temperature. (C) For a first order chemical reaction, the rate constant has unit of time-1. (D) Chemical kinetics can predict the rate of a chemical reaction. 2. In a chemical reaction, represented by A → P, it is observed that the rate of reaction increases by a factor of 4 on doubling the concentration of the reactant. The rate of reaction increases by a factor of 9 on trebling the concentration of the reactant. Then the rate of the reaction is proportional to (A) CA (B) CA2 (C) CA3 (D) CA4 3. An elementary reaction has the stoichiometric equation A + 2B = P. What is the order of reaction (A) 0 (B) 1 (C) 2 (D) 3 4. It states that the rate of a chemical reaction is directly proportional to the product of the activities or concentrations of the reactants. (A) Law of mass action…arrow_forwardThe isomerization of cyclopropane, C3H6, to propylene, CH2=CHCH3, is first order in cyclopropane and first order overall. At 1000oC, the rate constant is 9.2/s. (a) What is the half-life of cyclopropane at 1000oC? (b) How long would it take for the concentration of cyclopropane to decrease to 50% of its initial value? (c) To 25% of its initial value?arrow_forward
- For the reaction: 2N205(g) -->4NO(g) + O2(g) (a) write the mathematical rate expression in terms of (i) the disappearance of N2O5 (Reactant); (ii) the formation of NO (Product); (iii) the formation of O2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)arrow_forwardAcetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first-order process to methane and ketene (CH2═C═O). At 600°C, the rate constant is 8.7 × 10−3 s−1. (a) What is the half-life of the reaction? Give your answer in scientific notation. (b) How long does it take for 38% of a sample of acetone to decompose? (c) How long does it take for 81% of a sample of acetone to decompose? Give your answer in scientific notation.arrow_forward(a) Describe the term “integrated rate law” and briefly explain how it can be used tographically obtain the order of a reaction. (4)(b) Define the term “half-life of a substance” and briefly explain how it be used todetermine the order of the reaction and the rate constant for a first-order reaction. (4)arrow_forward
- The reaction A + B → P is found to be first order in both A and B. The reaction was carried out in a solution that was initially 0.080 mol dm−3 in A and 0.060 mol dm−3 in B. After 1.0 h the concentration of B had fallen to 0.030 mol dm−3. (i) Calculate the rate constant. (ii) What are the half-lives of the reactants?arrow_forward(a) A reaction is second order in A and first order in B.(i) Write the differential rate equation.(ii) How is the rate affected on increasing the concentration of A three times?(iii) How is the rate affected when the concentrations of both A and B are doubled?(b) A first order reaction takes 40 minutes for 30% decomposition. Calculate t1/2 for this reaction. (Given: log 1.428 = 0.1548)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
- Many drugs decompose in blood by a first-order process.(a) Two tablets of aspirin supply 0.60 g of the active compound.After 30 min, this compound reaches a maximum concentra-tion of 2 mg/100 mL of blood. If the half-life for its break-down is 90 min, what is its concentration (in mg/100 mL) 2.5 h after it reaches its maximum concentration?(b) For the decomposition of an antibiotic in a person with a nor-mal temperature (98.6°F), k=3.110⁻⁵s⁻¹; for a person witha fever at 101.9°F, k=3.910⁻⁵s⁻¹. If the person with thefever must take another pill when of the first pill has decom-posed, how many hours should she wait to take a second pill? A third pill? (Assume the pill is effective immediately.)(c) Calculate Eₐ for decomposition of the antibiotic in part (b)arrow_forwardThe decomposition of a certain insecticide in water at 12oC follows first-order kinetics with a rate constant of 1.45 yr-1. A quantity of this insecticide is washed into a lake on June 1, leading to a concentration of 5.0 x 10-7 g/cm3. Assume that the average temperature of the lake is 12oC. (a) What is the concentration of the insecticide on June 1 of the following year? (b) How long will it take for the insecticide concentration to decrease to 3.0 x 10-7 g/cm3?arrow_forward!arrow_forward
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