Question

Q: The activation energy of one of the reactions in a biochemical process is 87 kJ mol-1. The change in rate constant when thetemperature falls from 37°C to 15°C is?076​

Answer 1

The change in rate constant is 13.2

• The rate equation illustrates how altering the reactant concentrations affects the rate of the reaction. What about all the additional factors that affect reaction rates, such as temperature and catalysts, for instance? What role do these play in this formula?
• All of these are incorporated into the so-called rate constant, which is only really constant if the only variable changing is the reactant concentration. The rate constant varies, for instance, when the temperature or the catalyst are changed. The Arrhenius equation provides a mathematical illustration of this.

Here, according to the given information, we are given that,

The activation energy of one of the reactions in a biochemical process is 87 kJ $mol^{-1}$.

Now, we know that,

$k = Ae^{-\frac{E_{a} }{RT} }$

Now, if ratios are taken, we get,

$\frac{k_{1} }{k_{2} } = Ae^{-\frac{E_{a} }{R}(\frac{1}{t_{1} }-\frac{1}{t_{2} }) }$

Or, $\frac{k_{1} }{k_{2} } = Ae^{-\frac{E_{a} }{R}(\frac{1}{310 }-\frac{1}{288}) }$

Or, $k_{1} : k_{2} =13.2:1$

Hence, the change in rate constant is 13.2

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