C(diamond) → C(graphite) ΔG° = -2.9 kJ/mol_rxn Which of the following best explains why the reaction — Thermodynamics Chemistry Question
Question
C(diamond) → C(graphite) ΔG° = -2.9 kJ/mol_rxn
Which of the following best explains why the reaction represented above is not observed to occur at room temperature?
A.
The rate of the reaction is extremely slow because of the relatively small value of ΔG° for the reaction.
B.
The entropy of the system decreases because the carbon atoms in graphite are less ordered than those in diamond.
C.✓ Correct
The reaction has an extremely large activation energy due to strong three-dimensional bonding among carbon atoms in diamond.
D.
The reaction does not occur because it is not thermodynamically favorable.
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