Question

From the standard enthalpies of formation values for some compounds (in kJ mol^{-1}), predict which one of them will be most stable?

• A. Propane $\left(g\right)\left(\Delta H^{\circ}_{f}=-103.8\right)$
• B. n-Butane $\left(g\right)\left(\Delta H^{\circ}_{f}=-124.7\right)$
• C. n-Butane $\left(g\right)\left(\Delta H^{\circ}_{f}=-167.2\right)$
• D. n-Octane $\left(g\right)\left(\Delta H^{\circ}_{f}=-208.4\right)$

Answer 1

Answer: (D)

Greater the standard enthalpy of formation, the more stable will be the compound