Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.
(N/A) The combustion of fuels is a chemical reaction that requires a certain minimum amount of energy,known as the activation energy $(E_a)$,to initiate the process. At room temperature,the average kinetic energy of the fuel molecules is significantly lower than the required activation energy. Therefore,the molecules do not possess sufficient energy to overcome the energy barrier,and the reaction does not occur spontaneously.
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The decomposition of $N_2O$ into $N_2$ and $O_2$ in the presence of argon follows first-order kinetics. If the rate constant is given by $K = 5.0 \times 10^{11} \, e^{-2000/T}$,what is the activation energy of the reaction?
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Which scientist explained that all the species taking part in a reaction do not possess the same kinetic energy?
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Among the following graphs showing the variation of rate constant $(k)$ with temperature $(T)$ for a reaction,the one that exhibits Arrhenius behaviour over the entire temperature range is:
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