JEE Advance - Chemistry (2017 - Paper 2 Offline - No. 11)
In a bimolecular reaction, the steric factor $$P$$ was experimentally determined to be $$4.5.$$ The correct option(s) among the following is (are)
The activation energy of the reaction is unaffected by the value of the steric factor
Experimentally determined value of frequency factor is higher than that predicted by arrhenius equation
Since $$P = 4.5,$$ the reaction will not proceed unless an effective catalyst is used
The value of frequency factor predicted by Arrhenius equation is higher than that determined experimentally
Explanation
Arrhenius equation is
$$k = A{e^{ - {E_a}/RT}}$$
where, A = Frequency factor
Taking into account orientation factor,
$$k = P{Z_{AB}}{e^{ - {E_a}/RT}}$$
where, P = steric factor, ZAB = collision frequency
The value of steric factor lies between 0 and 1 predicted by Arrhenius equation. Thus, the experimentally determined value of frequency factor is higher than that predicted by Arrhenius equation.
The activation energy of the reaction does not depend upon the value of the steric factor.
If P is very small, then catalyst is required to carry out the reaction at measurable rate.
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