In a reaction carried out at 400K , 0.01 % of the total number of collisions is effective. The energy of activation of the reaction is

Question

In a reaction carried out at 400K , 0.01 % of the total number of collisions is effective. The energy of activation of the reaction is (A) 13.3kJ/mol (B) 23.5kJ/mol (C) 3.2kJ/mol (D) 30.6kJ/mol

Tardigrade Admin · Accepted Answer

K=Ae- (Ea/R T) e(Ea/R T)=(0.01/100)⇒ (Ea/R T)=2.303log 10- 4 ⇒ Ea=2.303× 4× 400=30.6kJ/mol

Q. In a reaction carried out at $400 K$ , $0.01%$ of the total number of collisions is effective. The energy of activation of the reaction is

$13.3 k J / m o l$

$23.5 k J / m o l$

$3.2 k J / m o l$

$30.6 k J / m o l$

$K = A e^{- \frac{E _{a}}{RT}}$

$e^{\frac{E _{a}}{RT}} = \frac{0.01}{100} \Rightarrow \frac{E _{a}}{RT} = 2.303 l o g 1 0^{- 4}$

$\Rightarrow E_{a} = 2.303 \times 4 \times 400 = 30.6 k J / m o l$

Q. In a reaction carried out at 400K , 0.01% of the total number of collisions is effective. The energy of activation of the reaction is

13.3kJ/mol

23.5kJ/mol

3.2kJ/mol

30.6kJ/mol