The reaction between $H_{2(g)}$ and $O_{2(g)}$ is highly feasible,yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of water. Explain.
(N/A) The reaction is thermodynamically feasible because the Gibbs free energy change $(\Delta G)$ is negative.
However,the reaction does not occur at room temperature because the activation energy $(E_a)$ required to break the strong $H-H$ and $O=O$ bonds is very high.
At room temperature,the number of molecules possessing energy equal to or greater than the activation energy is negligible.
Therefore,despite frequent collisions,the effective collisions are insufficient to form the product,water.
However,the reaction does not occur at room temperature because the activation energy $(E_a)$ required to break the strong $H-H$ and $O=O$ bonds is very high.
At room temperature,the number of molecules possessing energy equal to or greater than the activation energy is negligible.
Therefore,despite frequent collisions,the effective collisions are insufficient to form the product,water.
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