Match the statements given in Column I and Column II
Column I Column II
(i) Catalyst alters the rate of reaction (a) cannot be fraction or zero
(ii) Molecularity (b) proper orientation is not there
Always
(iii) Second half life of first order reaction (c) by lowering the activation
Energy
(iv) e–Ea/R T (d) is same as the first
(v) Energetically favourable reactions are sometimes slow (e) total probability is one
(vi) Area under the Maxwell Boltzman curve is constant (f) refers to the fraction of molecules with energy equal
to or greater than activation
energy
(i)→(c),(ii) → (a),(iii) → (d),(iv) → (f),(v) → (b),(vi) → (e)
(i) →(c), A catalyst provides an alternate path of reaction with a lower activation energy between the reactant and the product. Thus, lowering the potential energy barrier.
(ii)→(a), Molecularity of a reaction is the number of reacting species (atoms, molecules) taking part in an elementary reaction that must collide in order to bring about a chemical reaction.
Thus, for an elementary reaction taking place molecularity cannot be zero or fraction for it.
(iii) → (d), the first half-life of a first-order reaction is, t_(1/2)=.693/k.
For the second half-life of the first-order reaction, the initial concentration of reactant after the first half-life is R_0/2 , the final concentration of reactant after the second half-life is R_0/4 .
Thus, putting these values in the equation
log〖 [R]〗=-kt/2.303+log[R_0]
Where K is the rate constant, R is the final molar concentration of a reactant and R0 is the molar concentration of a reactant initially.
We get,
t_(1/2)=0.693/k
Hence, the second half-life of the first-order reaction is equal to the first half-life of the first-order reaction.
(iv) →(f), An Arrhenius equation i.e. k=Ae^(-E_a/RT) .
Where A is the frequency factor and term e^(-E_a/RT) corresponds to the fractions of molecules having kinetic energy equal to or greater than the activation energy.
(v) →(b), An Arrhenius equation i.e. k=Ae^(-E_a/RT) .
Where A is the frequency factor and term e^(-E_a/RT) corresponds to the fractions of molecules having kinetic energy equal to or greater than the activation energy.
Thus even if the reaction is an energetically favorable reaction but if there is not the proper orientation between the collision of the molecules the reaction will be slow.
(vi) →(e), Area under the Maxwell Boltzman curve is constant as the total probability is one.
The above statement means that the sum energies of all molecules involved in a reaction remain constant even on increasing the temperature.
The most probable energy of molecules decreases due to the increased in the collision between molecules but the number of molecules with activation energy EA increases due to the increase in temperature.
Thus, the total energy remains constant.