Question

Calculate ∆H for the conversion of graphite to diamond . Heats of combustion of graphite and diamond measured at 25°C and 1 atm pressure are-393.5kj and-395.4 kj respectively .​

Answer 1

Explanation:

Carbon occurs in two forms: graphite and diamond. The enthalpy of combustion of graphite is -393.5 kJ, and that of diamond is -395.4 kJ

C(graphite)+O

2

(g)→CO

2

(g)H=−393.5kJ

C(diamond)+O

2

(g)→CO

2

(g)H=−395.4kJ

C(graphite)→C(diamond)ΔH=+1.9kJ

Answer 2

Answer:

Carbon occurs in two forms: graphite and diamond. The enthalpy of combustion of graphite is -393.5 kJ, and that of diamond is -395.4 kJ.

C(graphite) + O2 → CO2(g) H = - 393.5 kj

C(diamond) + O2 → CO2(g) H = -395.4 kj

C(graphite) → C (diamond) )ΔH=+1.9kJ