Active Module: REACTION RATE
⚡
Reaction Rates & Collision Theory Simulator
Reactions require sufficient kinetic energy (E ≥ Ea) and favorable collision orientation.
Reaction Vessel: A (Red) + B (Blue) ➔ Product C (Green)
Reactant AReactant B
Potential Energy ProfileEa: 55 kJ
Total Collisions
142
Successful Hits
38
Products Formed
19
Rate Index
1 / 100
Temperature:310 K
Reactant Concentration:1 M
Surface Area (Solid Reactant):
📐Step-by-Step Mathematical Derivation
Given ➔ Formula ➔ Solve1. Given Quantities:
• Temperature: 310 K (37 °C)
• Concentration: [A] = 1 M, [B] = 1 M
• Surface Area: CHUNKS
• Catalyst: None (Ea = 55 kJ/mol)
2. Governing Formula:
Rate = Z · f · p (Collision Theory: Frequency × Energy Fraction × Orientation)
3. Substitute Values:
Collision Factor = 2.55 | Activation Energy Ea = 55 kJ/mol
4. Calculated Result:
Relative Reaction Rate Index = 1 / 100
5. Chemical Interpretation:Increasing temperature speeds molecular collisions and exponentially increases the proportion of collisions exceeding the activation energy threshold.
🔬Why Only Some Collisions React
Molecules collide billions of times per second, but most simply bounce off elastically!
A chemical reaction occurs only when colliding particles possess kinetic energy equal to or greater than the activation energy ($E \ge E_a$) and collide with correct molecular orientation.