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The given reaction is a heterogeneous reaction involving a solid reactant C(s) and a gaseous reactant O2(g). In chemical kinetics, the rate of reaction depends on the concentration of species in the gaseous or aqueous phase.
For the reaction C(s) + O2(g) → CO2(g), the rate law is expressed as: $$Rate = k[O_2]^1$$ The concentration of the solid C(s) is taken as unity (constant) and is incorporated into the rate constant.
The rate constant k cannot be determined solely from the chemical equation without experimental data (initial concentration and rate at a specific time). It is defined by the Arrhenius equation: $$k = Ae^{-E_a/RT}$$ Where A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature.
Final Answer: The rate constant k is determined experimentally using the Arrhenius equation k = Ae^{-E_a/RT} and cannot be calculated from the stoichiometry of the reaction alone.
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