5.6 - HL: The Temperature Dependence of Rate: The Arrhenius Equation and Activation Energy
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Practice Questions
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What is the Arrhenius equation used for?
💡 Hint: Think about reaction rates and temperature.
What is the universal gas constant value in the Arrhenius equation?
💡 Hint: It’s a constant used for calculations in chemistry.
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Interactive Quizzes
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What does the Arrhenius equation model?
💡 Hint: Recall the topics we've covered on reaction kinetics.
True or False: Higher activation energy means a faster reaction rate.
💡 Hint: Consider the meaning of activation energy.
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Challenge Problems
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The rate constant for a chemical reaction is known to increase from 3.0 x 10^-5 to 1.2 x 10^-4 s^-1 as the temperature rises from 298 K to 308 K. Using the Arrhenius equation, calculate the activation energy (Ea).
💡 Hint: Find the natural log of the ratio of the rate constants and set up the equation to solve for Ea.
A chemical reaction has an activation energy of 50 kJ/mol. How much faster will the reaction be at 350 K compared to 300 K based on the Arrhenius equation?
💡 Hint: Set up your calculations carefully, remembering to convert kilojoules to joules for R.
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