C(graphite) + O2(g) → CO2(g) + 94.05 kcal

C(diamond) + O2(g) → CO2(g) + 94.50 kcal

What could you infer from the information given above? Select all that apply.

A) The enthalpy of CO2 is greater than the reactants.
B) E2 - E1 is negative.
C) Graphite and diamond have equal enthalpy.
D) Diamond must have lower internal energy.

Question

C(graphite) + O2(g) → CO2(g) + 94.05 kcal

C(diamond) + O2(g) → CO2(g) + 94.50 kcal

What could you infer from the information given above? Select all that apply.

A) The enthalpy of CO2 is greater than the reactants.
B) E2 - E1 is negative.
C) Graphite and diamond have equal enthalpy.
D) Diamond must have lower internal energy.

sweetburger · Answer

That diamond is hard af to blow up.

aaronq · Answer

in this case the energy is shown as positive because it's part of the products, burning anything is exothermic. this reaction is NOT endothermic.

Combustion reactions be written as:
$\sf A+O_2\rightarrow C+\Delta H$
$\sf A+O_2\rightarrow C$       ; $\sf \Delta H=-ve$

The right answer should be B because $H_{products}<H_{reactants}$ and therefore $\Delta H$ is negative.