Please help!! I'm very confused about what equation I should be using. Not sure if I should be using the Arrhenius equation or not.?
2H2O2(aq)---> 2H2O(l) + O2(g)
The activation energy for this reaction is 75 kJxmol^-1. In the presence of a metal catalyst the activation energy is lowered to 49 kJxmol^-1.
At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal catalyzed reaction at 25 degrees C?
- GeorgeSiO2Lv 73 years ago
Arrhenius Equation 
Rate = Aexp-Ea1/RT
Ea = Activation energy in J mol^-1; R = 8.314 J mol^-1 K^-1; T in K
Rate(cat) = Aexp-(49000/(8.314×298.2) = Aexp-(19.76) = A(2.609×10^-9)
Rate(ucat) = A exp-(75000/(8.314×T)
(2.609×10^-9) = exp-(75000/(8.314×T) (A’s cancel)
ln of both sides
-19.76 = -75000/(8.314×T)
T = 75000/(19.76×8.314) = 456.4 – 273.2 = 183°C
- AlLv 73 years ago
This has NOTHING to do with Arrhenius.