This problem is only appropriate if you have taken calculus. For a zero-order reaction described by the chemical equation aA products the rate expression is dA adt where A is the reactant concentration, a is the coefficient of the reactant in the balanced chemical equation, and k is the rate constant. Ao = = k Derive the integrated rate expression for a zero-order reaction. Express your answer as an algebraic formula in terms of the variables A, a, k, and t. Incorrect At+ akt A plot of A versust would be linear for a zero-order reaction.

This problem is only appropriate if you have taken calculus. For a zero-order reaction described by the chemical equation aA products the rate expression is dA adt where A is the reactant concentration, a is the coefficient of the reactant in the balanced chemical equation, and k is the rate constant. Ao = = k Derive the integrated rate expression for a zero-order reaction. Express your answer as an algebraic formula in terms of the variables A, a, k, and t. Incorrect At+ akt A plot of A versust would be linear for a zero-order reaction.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 112QRT

See similar textbooks

Similar questions

A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
The 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)?
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.
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?
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
If you know some calculus, derive the integrated first-order rate law for the reaction by following these steps: Define the reaction rate in terms of [A]. Write the rate law in terms of [A], k, and t. Separate variables in the rate law. Integrate the rate law. Write the integrated equation in the form . Derive the half-life as was done in Section 11-3c.
If a reaction has the same rate constant, what time does it take for a reactant to decrease by 5 that is, still near the beginning of the reaction process if the kinetics are zeroth-order, first-order, and second-order with respect to that reactant?
As with any drug, aspirin (acetylsalicylic acid) must remain in the bloodstream long enough to be effective. Assume that the removal of aspirin from the bloodstream into the urine is a lirst-order reaction, with a half-life of about 3 hours. The instructions on an aspirin bottle say to take 1 or 2 tablets every 4 hours. If a person takes 2 aspirin tablets, how much aspirin remains in the bloodstream when it is time for the second dose? (A standard tablet contains 325 mg of aspirin.)
The gas-phase reaction of nitrogen monoxide with chlorine proceeds to form nitrosyl chloride. 2NO(g)+Cl2(g)2NOCl(g)rate=k[NO]2[Cl]2 Evaluate the following proposed mechanism to determine whether it is consistent with the experimental results, and identify intermediates, if any. 2NOk1k1N2O2Fast,reversibleN2O2(g)+Cl2(g)2NOCl(g)Slow(rate-limiting)step