🌟 Sizzling Fact: Did you know that Svante Arrhenius, the scientist who gave us the Arrhenius equation, was also the first to suggest that CO2 could lead to global warming? Talk about diverse achievements!

🔍 Equation: k = A × e−RTEa​

• k = rate constant.
• A = Arrhenius factor (or frequency factor).
• e = base of natural logarithms (≈ 2.718…).
• Ea = activation energy of the reaction.
• R = ideal gas constant.
• T = absolute temperature.

🌎 Real-world example: It's like trying to light a fire. The energy required to get the fire started (like striking a match) is akin to the activation energy. The temperature affects how quickly the wood catches fire (the rate).

• Specific for each reaction.
•  Reflects frequency & proper mutual orientation of colliding reactant particles
• . Larger the molecule, harder the angle: Bigger molecules need a specific angle to react, hence a lower A value.
• Units: Same as the rate constant k.

🍿 Popcorn Analogy: Imagine shaking a popcorn bag. When you shake harder (increased frequency and proper orientation), you get more popped corn!

• k values increase exponentially with temperature.
• You can determine activation energy by examining the rate constant's temperature dependence.

🔥 Hot Tip: Reaction rates generally double or triple for every 10°C rise in temperature!