question 4\nif the δg of the reaction that changes diamonds to graphite is -693 kcal/mol, then the reaction…
question 4\nif the δg of the reaction that changes diamonds to graphite is -693 kcal/mol, then the reaction is\na spontaneous and endergonic\nb spontaneous and exergonic\nc not spontaneous and exergonic\nd not spontaneous and endergonic
Answer
Brief Explanations:
The sign of $\Delta G$ determines reaction spontaneity. A negative $\Delta G$ indicates a spontaneous reaction. Exergonic reactions release energy ($\Delta G < 0$) and endergonic reactions absorb energy ($\Delta G>0$). Since $\Delta G=- 693$ kcal/mol (negative), the reaction is spontaneous and exergonic.
Answer:
B. spontaneous and exergonic