Collision Theory of Chemical Reactions
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- According to Arrhenius equation, rate of reaction increases with increase in temp. Give reasons.
Ans. With increase in temp. the kinetic energy of the molecules increases. So that number of effective collision increases giving more product. Hence rate of reaction increases.
- How is rate constant related to conc. of the reactant ?
Ans. Rate constant is independent of conc. of
- Write two factors which influence the rate of reaction.
Ans. Concentration of reactant and tempeature.
4. What is the order of overall reaction ?
Ans. Order is deternmined from the slowest step. So order of the reaction is
- What is the unit of rate constant for 2nd order reaction ?
Ans. Mole–¹ lit sec–¹
- Calculate order of the reaction having rate expression, rate = K[A]2[B]3
Ans. Order = 3/2 + 1/2 = 2
- Give an example of zero order reaction.
Ans. Decomposition of ammonia giving nitrogen and hydrogen in presence of Pt–catalyst at 800° is an
example of zero order reaction.
2NH³ N²+ 3H²
Rate K [NH³] ⁰
- Express the rate of reaction for the reaction A, + 3B–→ 2AB³ in terms of reactants and products.
Ans. Rate of reaction
=dA²/dt = – 1/3 (d)B²/ dt=+ 1/2 d[AB³]/dt
- Define rate of reaction.
Ans. It is defined as the amount of reactant
Consumed or amount of product formed per unit time.
Rate of reaction=-(DX/dt) (w.r.t. reactant)= +(dx/dt) w. r.t. product)
- What is the relationship between activation energy and threshold energy ?
Ans. Eà= Eth-ER
Where Eà =activation energy of reactant
Eth= threshold energy
ER = average kinetic energy of reactant.