⚡ Reaction Rate & Collision Theory Simulator
Chemical KineticsWhat's happening? Rate ∝ [A][B] × e^(-Ea/RT). Higher temperature = faster molecules = more collisions. Catalyst lowers activation energy = 10× faster. Watch the collision flashes!
Kinetics: 4-6 questions every year.
JEE tests rate laws, order, half-life, Arrhenius equation.
Key formulas
Reaction Rate & Collision Theory Formulas
Rate law
Rate = k[A]^m[B]^n
m+n = overall order
First-order
ln[A]0/[A] = kt, t_1/2 = 0.693/k
Half-life independent of [A]0
Second-order
1/[A]-1/[A]0 = kt, t_1/2 = 1/(k[A]0)
Half-life depends on [A]0
Arrhenius
k = Ae^(-Ea/RT)
ln k vs 1/T: slope = -Ea/R
Step-by-step problem solving
How to solve chemistry problems in JEE
- Determine order from data
- Write integrated rate equation
- Solve for k, [A], or t_1/2
- Arrhenius: ratio or plot
Common JEE mistakes
What students get wrong
Order = coefficients
Order is experimental, not from equation
Wrong half-life
1st: 0.693/k, 2nd: 1/(k[A]0)
Negative ln
Check if you swapped [A]0 and [A]
Units of k
1st: s^-1, 2nd: L/mol*s, 0th: mol/L*s
FAQs
Reaction Rate & Collision Theory Questions
Determine order from table?
Double [A], see if rate doubles (order 1) or quadruples (order 2)
Pseudo-first-order?
One reactant in excess, its [A] stays constant
Arrhenius plot?
ln k = ln A - Ea/(RT). Straight line.
Activation energy?
Minimum energy for effective collision. Catalysts lower it.