I carried a calculation through on this one using the two-point Arrhenius equati

Question

I carried a calculation through on this one using the two-point Arrhenius equation, but my prof emailed us and said that we may need the enzyme concentration, which is [E] = 4.00 x 10^-9 M. Does this change my calculation, and if so, how do I account for [E]?

The rate of the oxidation of ethanol by horse liver alcohol dehydrogenase has been studied from 0 degree C up to 20 degree C, yielding the following data, all collected at saturating concentrations of ethanol and NAD+. What is the activation energy for this hydride transfer reaction?

Explanation / Answer

rate = A exp[-Ea/RT]

so we apply this for two different cases

o.23 = A exp-[Ea/R*273]-------[1]

0.32 =Aexp-[Ea/R*278]------[2]

dividing both the equations we get and taking ln on both sides

ln [0.23/0.32]= Ea/R[1/278-1/273]

=-0.33 = Ea /R [-6.5*10^-5]

Ea = 42209.53 J

friend i dont think so we need the conc of E anywhere as without the help f conc we can easily find out the activtion energy

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