Which of the following statements is correct about a half-life?a) For a second-order reaction, its half-life is independent of the initial reactant concentration.b) For a first-order reaction, its half-life is dependent on the initial reactant concentration.a) onlyO b) onlyBoth a) and b) are correct.O Neither a) nor b) is correct

The half-life of a chemical reaction is the time it takes for a particular reactant's concentration…

Answered: Which of the following statements is…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 21QAP: The reaction ICl(g)+12 H2(g)12 I2(g)+HCl(g)is first-order in both reactants. At a certain...

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One can also define a third-life, t1/3, which is the amount of time necessary for one-third of an original amount of reactant to react. a For which order of kinetics is the third-life a constant? b Derive an expression for the t1/3 of a zeroth-order reaction. For how many third-lives will the reaction proceed before completion?
When a base is added to an aqueous solution of chlorine dioxide gas, the following reaction occurs: 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O The reaction is first-order in OH and second-order for ClO2 Initially, when [ ClO2 ]=0.010M and [ OH ]=0.030M, the rate of the reaction is 6.00104mol/Ls. What is the rate of the reaction when 50.0 mL of 0.200 M ClO2 and 95.0 mL of 0.155 M NaOH are added?
In a first-order reaction, suppose that a quantity X of a reactant is added at regular intervals of time, t. At first the amount of reactant in the system builds up; eventually, however, it levels off at a saturation value given by the expression a saturation value saturationvalue= x110a where a=0.30tt1/2 This analysis applies to prescription drugs, of which you take a certain amount each day. Suppose that you take 0.100 g of a drug three times a day and that the half-life for elimination is 2.0 days. Using this equation, calculate the mass of the drug in the body at saturation. Suppose further that side effects show up when 0.500 g of the drug accumulates in the body. As a pharmacist, what is the maximum dosage you could assign to a patient for an 8-h period without causing side effects?
The reaction ICl(g)+12 H2(g)12 I2(g)+HCl(g)is first-order in both reactants. At a certain temperature, the rate of the reaction is 2.86105mol/Ls when [ ICl ]=0.0500M and [ H2 ]=0.0150M. (a) What is the value of k at that temperature? (b) At what concentration of hydrogen is the rate 2.66104mol/Ls and [ ICl ]=0.100M? (c) What is [ ICl ] when the rate is 0.0715mol/Ls and H2=3[ ICl ]?
Derive an expression for the half-life of a a third order reaction;b a reaction whose order is =1; c a reaction whose order is 12. In these last two cases, examples are rare but known.
The uncoiling of deoxyribonucleic acid (DNA) is a first-order reaction. Its activation energy is 420 kJ. At 37C, the rate constant is 4.90104min1 (a) What is the half-life of the uncoiling at 37C (normal body temperature)? (b) What is the half-life of the uncoiling if the organism has a temperature of 40C(104F)? (c) By what factor does the rate of uncoiling increase (per C) over this temperature interval?
The reaction is catalyzed by the enzyme succinate dehydrogenase. When malonate ions or oxalate ions are added to the reaction mixture, the rate decreases significantly. Try to account for this observation in terms of the description of enzyme catalysis given in the text. The structures of malonate and oxalate ions are
Consider the first-order decomposition reaction A+BCwhere A (circles) decomposes to B (triangles) and C (squares). Given the following boxes representing the reaction at t=2 minutes, fill in the boxes with products at the indicated time. Estimate the half-life of the reaction.
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
Consider a set of first-order consecutive reactions ABC. The rate constants are 8.4104s1 and 3.02105s1, respectively. Plot the concentrations of A, B, and C versus time, and determine the time necessary to produce the maximum amount of the intermediate product B.
Consider a reaction that has two parallel pathways both first-order to products. Pathway 1, leading to product B, has a rate constant of 1.34105s1. Product C- producing pathway 2 has a rate constant of 6.55104s1. Plot the concentrations of A, B, and C versus time, and determine the time necessary to produce the maximum amount of the kinetically favored product.
Nitric oxide, NO, is known to break down ozone, O3, by the following bimolecular reaction: NO(g)+O3(g)NO2(g)+O2(g) If the activation energy of this reaction is 10.5kJ/mol and the pre-exponential factor is 7.91011cm3/(mols), a what is the rate constant of this reaction at 298K? b If the ozone concentration were 5.41012mol/cm3 and the NO concentration were 2.01012mol/cm3 conditions that might exist in a high-pollution area, what is the rate of this reaction?

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