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On the basis of enthalpy of formation, g...

On the basis of enthalpy of formation, graphite is more stable than diamond, yet diamond does not change into graphite for years. Why ?

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The activation energy for the reaction C (diamond)`to` C (graphite) is very high which is not available at room temperature.
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Thermodynamically graphite is more stable than diamond but diamond does not transform into graphite on its own. Why?

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Knowledge Check

  • Diamond is harder than graphite because

    A
    Graphite is planar
    B
    Diamond has free electron
    C
    Graphite is `sp^(3)` hybridised
    D
    None of these

  • Diamond and graphite are the

    A
    isotopic forms of carbon
    B
    allotropic forms of carbon
    C
    amorphous forms of carbon
    D
    isometric forms of corbon

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