A) Calculate the half-life of the antimicrobial agent at 25°C. Be sure to include the units. B) The activation energy for the degradation reaction is 9.2 kJ mol-'. Sup- pose you store your sunscreen in the locker room at the gym, which has an average temperature of 35°C. What is the half-life of the an- timicrobial agent in the conditions at the gym?

A) Calculate the half-life of the antimicrobial agent at 25°C. Be sure to include the units. B) The activation energy for the degradation reaction is 9.2 kJ mol-'. Sup- pose you store your sunscreen in the locker room at the gym, which has an average temperature of 35°C. What is the half-life of the an- timicrobial agent in the conditions at the gym?

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...

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Enter your answer in the provided box. The rate at which tree crickets chirp is 2.20 × 102 per minute at 25°C but only 40.7 per minute at 6.5°C. From these data, calculate the activation energy for the chirping process. kJ/mol Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.
The reaction aA → products gives a plot of [A] vs time (in seconds) which is astraight line with a slope of -4.50×10–3. Assuming [A]0 = 0.200 M, how manyseconds are required for the reaction to reach 60.0% completion.
For the gas phase decomposition of acetic anhydride, (CH₂CO)₂0-CH₂-C-O + CH3COOH the rate constant in s¹ has been determined at several temperatures. Which of the following should give a linear plot (temperatures in K)? On the y-axis: k Use this information to determine the activation energy for the reaction. When the appropriate plot is made, the resulting least-squares line has a slope of -1.73x104 K and a y-intercept of 27.6. Submit Answer On the x-axis: Try Another Version 3 item attempts remaining v E₂ = kJ/mol
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Explain your reasoning, please. Thank you.
The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activation energy to 81 kJ/mol Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C? Express the ratio to two significant digits. Templates Symbols undo rego feset keyboard shortcuts Help k./k, = 23•106 Submit Prevlous Anawers Requeat Anawer X Incorrect; Try Again; 7 attempts remaining Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C? Express the ratio to two significant digits. Templates SymBols undo redo Teset keyboard shortcuts Help k/k = Submit Request Anewer < Return to Assignment Provide Feedback
d-f please only
A reaction increases its rate four times when temperature increases from 250 K to 300 K. What is the activation energy of the reaction? Round off your answer to 3 significant figures and with correct units:
The mechanism of the decomposition of hydrogen peroxide is H202(aq) + I-(aq) -> H2O(l) + IO-(aq) IO-(aq) + H202(ag) -> H20(l) + 02(9) + I- (aq) what is the overall reaction equation? is there a reaction intermediate? if so, what is it? Is there a catalyst? If so, what is it? what is the rate law for the overall reaction?
In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °CNH4NCO(aq)(NH2)2CO(aq)the following data were obtained: [NH4NCO], M 0.780 0.390 0.195 9.75×10-2 minutes 0 131 393 918 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.780 M is______ min and when the starting concentration is 0.390 M is ______min.(2)The average (1/[NH4NCO]) / t from t = 0 min to t = 131 min is______ M-1 min-1.The average (1/[NH4NCO]) / t from t = 131 min to t = 393 min is_____ M-1 min-1.(3)Based on these data, the rate constant for this _______ (zerofirstsecond) order reaction is M-1 min-1. fill in the blanks