For C(diamond) -%26gt; C(graphite), the standard gibbs free energy change has a value of -2.90 kJ/mol. Which of the following best accounts for the observation that the reaction does NOT occur (i.e diamond is stable ) at 298K and 1 atm?
(A) Delta S for the reaction is positive.
(b) The activation energy for the reaction is very large.
(c) The reaction is slightly exothermic
(d) Diamond has a density greater than that of graphite
(e) Diamond has a heat capacity lower than that of graphite.
For C(diamond) -%26gt; C(graphite), the standard gibbs free energy change has a value of -2.90 kJ/mol.?
B: The activation energy for the reaction is very large.
In order to change diamond into graphite you need to heat it until the bonds between the carbon atoms break. (Very high temperature = very high activation energy)
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