🤓 Based on our data, we think this question is relevant for Professor Waddell's class at UC.

Solution: Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25°C, diamond changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Using equations from the list below, determine ΔH  for C(diamond) ⟶ C(graphite)(1) C(diamond) + O2(g) ⟶ CO2(g)          ΔH = −395.4 kJ(2) 2CO2(g) ⟶ 2CO(g) + O2(g)              Δ H = 566.0 kJ(3) C(graphite) + O2(g) ⟶ CO2(g)          Δ H = −393.5 kJ(4) 2CO(g) ⟶ C(graphite) + CO2(g)      ΔH = −172.5 kJ