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cjones2941
24.11.2021 •
Chemistry
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Ответ:
The answer to the question is
The enzyme must lower the activation energy by 35624.5 KJ/mol
Explanation:
The relation is
k =![Ae^{\frac{-Ea}{RT} }](/tpl/images/0506/0037/b2fb0.png)
Where k = rate of chemical reaction
A = Arrhenius constant
Ea = Activation energy
T = Temperature
R = Gas constant
at 37 °C we have T = (37 +273.15) K = 310.15 K
k =![Ae^{\frac{-Ea}{(8.314)(310.15)} }](/tpl/images/0506/0037/68291.png)
when a catalyst is introduced we have Ea(catalyst)
kc =![Ae^{\frac{-Eacatalyst}{(8.314)(310.15)} }](/tpl/images/0506/0037/a9f0c.png)
Finding the ratio of the two reaction rate and noting that Kc/K = 1.0 x 10⁶
Thus we have
Kc/k =
= 1.0 x 10⁶ by taking natural logarithm of both sides, we have
6 × ln (10) = Ln (Kc/k ) =
so that Ea - Eacatalyst = 8.314 × 310.15 × 13.816 = 35624.5 KJ/mol
Therefore the enzyme must lower the activation energy by 35624.5 KJ/molto achieve a million fold increse in the reaction rate constant