24. We had a homework problem in which the Arrhenius equation was applied to the blinking of fireflies. Several other natural phenomena also obey that equation, including the temperature dependent chirping of crickets. A particular species, the snowy tree cricket, has been widely studied. These crickets chirp at a rate of 178 times per minute at 25.0°C, and the activation energy for the chirping process is 53.9 kJ/mol. What is the temperature if the |crickets chirp at a rate of 126 times per minute? (Please make sure to set up your solution clearly so you can receive some credit even if you do not make it all the way through to the result.)

24. We had a homework problem in which the Arrhenius equation was applied to the blinking of fireflies. Several other natural phenomena also obey that equation, including the temperature dependent chirping of crickets. A particular species, the snowy tree cricket, has been widely studied. These crickets chirp at a rate of 178 times per minute at 25.0°C, and the activation energy for the chirping process is 53.9 kJ/mol. What is the temperature if the |crickets chirp at a rate of 126 times per minute? (Please make sure to set up your solution clearly so you can receive some credit even if you do not make it all the way through to the result.)

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

Help please
Consider the Arrhenius plot below. 1/T If the equation of the line above has a slope of -7,970.289 and intercept of -19.083, what is the activation energy, E, in kJ/mol, of the reaction? Recall that the gas constant R is 8.314 J/(mol*K). In k
The activation energy (E,) for a certain biological reaction is 62.1 kJ/mol. If the rate constant (k) is 24.3 at normal body temperature (37°C), what is the rate constant during a fever (41°C)?
Consider the mechanism. step 1: step 2: overall: Which species is an intermediate? O AB A B3 B2 A + B₂ → AB + B₂ 2 2B₂ B AB + B B3 + A B3 + B Which species is a catalyst? B3 AB B₁ 2 B A
Calculate the activation energy for the reaction (in kJ/mol) when at 675 K the rate constant for the reaction shown below is 0.0000200, and at 109 K the rate constant is 0.00000800 .
Using the data in the plot below, calculate the value of the activation energy (in kJ/mol) for this reaction: 3.5 3 2.5 y= - 507.36x • 3.866 R'=0.9687 1.5 1 0.5 0.002 0.003 0.004 0.005 0.006 0.007 0.008 0.009 1/T (1/K)
If the rate of a reaction increases by a factor of 2.6 when the temperature is raised from 20 ∘C to 30 ∘C, the activation energy is is 71 kJ/mol. By what factor does the rate of this reaction increase when the temperature is raised from 120 ∘C to 130 ∘C?
The rate constant of a reaction is 5.00 s-1 at 270C. What will be the rate constant at 470C if the activation energy for the reaction is 75.0 kJ/mol? 1.15 s-1 32.7 s-1 0.0306 s-1 1.00 s-1
The activation energy for a certain reaction is +859 kJ/mol and AE for the reaction is -132 kJ/mol. WVhat is the activation energy for the reverse reaction?