Concept:The temperature coefficient of a reaction dictates how the rate changes with a standard increase in temperature.
Formula:$$ \frac{k_{(T + 10)}}{k_T} \approx 2 \text{ to } 3 $$
Solution:- According to collision theory and the Maxwell-Boltzmann distribution, raising the temperature by 10 K (or 10°C) slightly increases collision frequency but drastically increases the fraction of molecules possessing energy greater than the activation energy.
- For most standard homogeneous reactions, this specific 10 K increase causes the reaction rate to approximately double (increase by a factor of 2).
Why other options are incorrect:While it can sometimes triple in specific high-barrier reactions, 'double' is the standard, universally accepted rule of thumb in foundational kinetics.
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