When designing a consumer product, it is desirable for it to have a two-year shelf life. Often this means that the active ingredientin the product should not decrease by more than 5% in two years.If the reaction is first order, and the rate constant is: k = 2.56 × 10-2 yr 1, determine the half-life of an active ingredient that has ashelf life of 2.00 years.The half-life of an active ingredient is iyr.

Step 1: Step 2: Step 3: Step 4:

Answered: When designing a consumer product, it…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/s. Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq). How many seconds would be required for the initial concentration of Fe3+ to decrease to 12.5% of its initial value? Express your answer to two decijal positions.
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic…
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
SO2 Cl2 decomposes in the gas phase by the reaction SO, Cla (9) S02 (g) + Ch(9). Part A The reaction is first order in SO2 Ca and the rate constant is 3.0 x 106 s1 at 600 K. A vessel is charged with 3.0 atm of SO2 Ch at 600 K. The partial pressure of SO, Cl, at 3.0 x 10 s is atm. 1.2 O 0.81 O 1.1 x 105 2.7 0.23
Consider the mechanism. 2 A = B В +С — D Step 1: equilibrium Step 2: slow Overall: 2A +С — D Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =
Consider a hypothetical chemical reaction A + B → C, where A and B are reactants and C is the product. The reaction is known to have a high activation energy barrier. However, upon adding a catalyst, the reaction proceeds at a significantly faster rate. Explain the role of the catalyst in reducing the activation energy barrier and increasing the reaction rate.
A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104
Consider a reaction A → B with activation energy 50.7 kJ/mol. At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature. �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K �K=�∘C+273.15 1 kJ = 1000 J Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!
1a) A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 1.13×102 L mol-1 s-1 at 346.0°C and 3.55×103 L mol-1 s-1 at 548.0°C. Use the Arrhenius equation k = Ae-Ea/RT to: Calculate Ea for this reaction. 1b) Calculate the rate constant k at 416.0°C for this reaction. 1c) Calculate the pre-exponential factor A for this reaction.
The rate constant for a certain reaction is k = 2.00×10−3 s−1 . If the initial reactant concentration was 0.950 MM, what will the concentration be after 16.0 minutes?
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +F₂ (g) → NO₂F (g)+F (g) 2 F (g) + NO₂ (g) → NO₂F (g) Suppose also k₁ << k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = & rate constant k₁ k₂

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS