The rate constant of a reaction at 27° C is 2.3 × 10-3 min -1 and at this temperature 0.001 % of reactant molecules are able to cross the energy barrier existing between the reactants and the products. What is the maximum value of rate constant that can be achieved on raising the temperature?

Question

The rate constant of a reaction at 27° C is 2.3 × 10-3 min -1 and at this temperature 0.001 % of reactant molecules are able to cross the energy barrier existing between the reactants and the products. What is the maximum value of rate constant that can be achieved on raising the temperature? (A) 750 min -1 (B) 230 min -1 (C) 125 min -1 (D) 500 min -1

Tardigrade Admin · Accepted Answer

From Arrhenius equation log K= log A-(Ea/2.303 R T) Maximum value of K=A So, 'A' is maximum rate constant e - Ea / RT = Fraction of molecules crossing energy barrier =0.001 %=10-5 K=2.3 × 10-3 min -1 K = A e - Ea / R T 2.3 × 10-3 min -1= A × 10-5 2.3 × 102 min -1= A 230 min -1=A

$750 mi n^{- 1}$

$230 mi n^{- 1}$

$125 mi n^{- 1}$

$500 mi n^{- 1}$

Q. The rate constant of a reaction at 27∘C is 2.3×10−3min−1 and at this temperature 0.001% of reactant molecules are able to cross the energy barrier existing between the reactants and the products. What is the maximum value of rate constant that can be achieved on raising the temperature?

750min−1

230min−1

125min−1

500min−1

From Arrhenius equation logK=logA−2.303RTEa​​ Maximum value of K=A So, 'A' is maximum rate constant e−Ea/RT= Fraction of molecules crossing energy barrier =0.001%=10−5 K=2.3×10−3min−1 K=Ae−Ea/RT 2.3×10−3min−1=A×10−5 2.3×102min−1=A 230min−1=A

$750 mi n^{- 1}$

$230 mi n^{- 1}$

$125 mi n^{- 1}$

$500 mi n^{- 1}$