Explanation
Rate = K[A][B]2 Keeping [B] constant, [A] is made a 4 times, rate also become 4 times. Hence rate α [A] Keeping [A] constant, [B] is doubled, rate becomes 4 times. Hence rate α [B]2 ∴ rate = K[A][B]2
rate = K[A]2 [A] doubling, rate becomes four time. Hence rate α [A]2 [B] doubling, no effect on the rate. Hence rate α [B]0 ∴ rate = K[A]2[B]0
concentration of reactants
temperature is changed
H2 + Br2 → 2HBr
four times ∴ rate a [B]2
rate of zero order reaction is independent of the concentration of the reacting species
many bady collisions have a low probability
rate = K [A][B]2 Rate of reaction for slowest step
2 concentration increased = 10 times rate increased = 102 times ∴ Order = 2
There is no difference between order and molecularity of a reaction.
Both order and molecularity of a reaction are always the same.
∆H of reaction
100 Kj mole-1 ∆H = Ea - Ear - 30 = 70 - Ear ∴ Ear = 100
increasing the temperature
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