Question

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?2.85 × 104 s-1576 s-19.56 × 103 s-14.33 × 1087 s-11.36 × 102 s-1

Answer 1

k ≈ 9,56x10³ s⁻¹

Step-by-step explanation:

It is possible to solve this question using Arrhenius formula:

`ln(k2)/(k1) = (-Ea)/(R) ((1)/(T2) -(1)/(T1) )`

Where:

k1: 1,35x10² s⁻¹

T1: 25,0°C + 273,15 = 298,15K

Ea = 55,5 kJ/mol

R = 8,314472x10⁻³ kJ/molK

k2 : ???

T2: 95,0°C+ 273,15K = 368,15K

Solving:

`ln(k2)/(k1) = 4,257`

`(k2)/(k1) = 70,593`

`{k2} = 9,53x10^3 s^(-1)`

k ≈ 9,56x10³ s⁻¹

I hope it helps!