A certain reaction rate increases 1000 folds in the presence of a catalyst at 27° C. The activation energy of the original pathway is 98 kJ / mol. What is the activation energy of the new pathway?

Question

A certain reaction rate increases 1000 folds in the presence of a catalyst at 27° C. The activation energy of the original pathway is 98 kJ / mol. What is the activation energy of the new pathway? (A) 80.77 kJ (B) 56.38 kJ (C) 24.67 kJ (D) 90.43 kJ

Tardigrade Admin · Accepted Answer

log (k2/k1)= log 1000 =(E1-E2/R T) =(98000-E2/8.314 × 300) E2 (catalyst) =80.77 k J

Q. A certain reaction rate increases $1000$ folds in the presence of a catalyst at $2 7^{\circ} C$ . The activation energy of the original pathway is $98 k J / m o l$ . What is the activation energy of the new pathway?

80.77 kJ

56.38 kJ

24.67 kJ

90.43 kJ

$lo g \frac{k _{2}}{k _{1}} = lo g 1000$
$= \frac{E _{1} - E _{2}}{RT}$
$= \frac{98000 - E _{2}}{8.314 \times 300}$
$E_{2}$ (catalyst) $= 80.77 k J$

Q. A certain reaction rate increases 1000 folds in the presence of a catalyst at 27∘C. The activation energy of the original pathway is 98kJ/mol. What is the activation energy of the new pathway?