Thermodynamic feasibility of the reaction alone cannot decide the rate of the reaction. Explain with the help of one example.
(N/A) Thermodynamic feasibility (indicated by a negative value of Gibbs free energy change,$\Delta G < 0$) does not determine the rate of a reaction. $A$ reaction may be thermodynamically spontaneous,but its rate can be extremely slow due to a high activation energy $(E_a)$.
For example,the conversion of diamond to graphite is thermodynamically feasible ($\Delta G$ is negative),but the reaction is kinetically very slow at room temperature because it possesses a very high activation energy.
For example,the conversion of diamond to graphite is thermodynamically feasible ($\Delta G$ is negative),but the reaction is kinetically very slow at room temperature because it possesses a very high activation energy.
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