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Understanding Collision Theory and Activation Energy in Chemistry

Learn about collision theory, activation energy, temperature's effect on activation energy, and the Arrhenius Equation. Discover how to calculate activation energy using the Arrhenius Equation in its logarithmic form. Explore a chemical reaction example and the mathematical operation required to determine activation energy. Enhance your knowledge of chemistry with this insightful guide.

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Understanding Collision Theory and Activation Energy in Chemistry

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  1. Collision theory and Activation Energy

  2. Temperature and Activation Energy

  3.  Temperature and  in Ea

  4. Arrhenius Equation

  5. Arrhenius Equation You may also come across it in a different form created by a mathematical operation on the standard one: "ln" is a form of logarithm. Don't worry about what it means. If you need to use this equation, just find the "ln" button on your calculator.

  6. 2N2O5 (g)→4NO2 (g) + O2 (g)

  7. Finding Ea

  8. Ea = activation energy R = 8.314 J/mol·K T = absolute temperature in KelvinsA = frequency factor

  9. The Arrhenius equation is often written in the logarithmic form:

  10. Ea=-R(slope) • Slope =Δln(k)/Δ(1/T) • Ea=-(8.3145J/K*mol)(-12000K) • =100,000 J/mol

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