How Does Temperature Affect the Rate Constant of a Reaction?

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SUMMARY

The discussion focuses on calculating the rate constant of a reaction at different temperatures using the Arrhenius equation. Given an activation energy of 48 kJ/mol and a rate constant of 2.5 x 10-2 s-2 at 15 degrees Celsius, the calculated rate constant at 37 degrees Celsius is approximately 0.104 s-1. The participants utilized the equation ln(k1/k2) = [Ea/R] [(T1-T2)/(T1*T2)] and confirmed the conversion of temperatures to absolute and activation energy to J/mol for accurate calculations.

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  • Understanding of the Arrhenius equation
  • Knowledge of activation energy and its units
  • Familiarity with temperature conversion to Kelvin
  • Basic logarithmic functions and their properties
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  • Learn about the effects of temperature on reaction kinetics
  • Explore the concept of activation energy and its measurement
  • Investigate other factors affecting rate constants in chemical reactions
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Chemistry students, educators, and professionals involved in reaction kinetics and thermodynamics will benefit from this discussion.

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Homework Statement


given that activation energy for a certain reaction is 48 kJ/mol, and the rate constanct is 2.5 x 10-2 s-2 at 15 degrees Celsius. what is the rate constant at 37 degrees Celsius?



Homework Equations


ln k1/k2 = [Ea/R] [(T1-T20)/(T1*T2)]


The Attempt at a Solution


my answer is k1= .1037740579 = .104 s-1


thank you for all the help!
 
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Converting all temperatures to absolute and 48kJ to 48000 J so the units on the gas constant cancel I came up with 5.3*10^-3 s^-2

I used this equation:

ln k1/ln k2 = Ea/R(1/T2-1/T1)
 

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