For the following reaction,
`{:(C("diamond")+O_(2)to CO_(2)(g),, DeltaH=-97.6kcal),(C("graphite")+O_(2)to CO_(2)(g),,DeltaH=-94.3kcal):}`
The heat change for the conversion of 1 g of C (diamond) to C(graphite) is:

For the following reaction, C_("diamond")+O_(2)toCO_(2)(g), DeltaH=-94.3" "kcal C_("graphite")+O_(2)toCO_(2)(g), DeltaH=-97.6" "kcal the heat require to change 1 g of C_("diamond")toC_("graphite") is:

C_(("graphite")) + O_(2(g)) to CO_(2(g)) - 94.0 kcal

C(s)+O_(2)(g)toCO_(2)(g),DeltaH=-94 kcal 2CO(g)+O_(2)to2CO_(2),DeltaH=-135.2 kcal The heat of formation of CO(g) is

C(s)+O_(2)(g)toCO_(2)(g),DeltaH=-94 kcal 2CO(g)+O_(2)to2CO_(2),DeltaH=-135.2 kcal The heat of formation of CO(g) is

Calculate the heat of transition for carbon from the following: C_("Diamond") +O_(2) rarr CO_(2)(g),DeltaH =- 94.3 kcal C_("Amorphous") +O_(2) rarr CO_(2)(g),DeltaH =- 97.6 kcal Also calculate the heat required to change 1g of C_("Diamond") to C_("Amorphous") .

Calculate the heat of transition for carbon from the following: C_("Diamond") +O_(2) rarr CO_(2)(g),DeltaH =- 94.3 kcal C_("Amorphous") +O_(2) rarr CO_(2)(g),DeltaH =- 97.6 kcal Also calculate the heat required to change 1g of C_("Diamond") to C_("Amorphous") .

The enthalpy change for the following reactions are: C_("diamond")+O_(2(g)) rarr CO_(2(g))" "DeltaH=-395.3 KJ "mol"^(-1) C_("graphite")+O_(2(g)) rarr CO_(2(g)) " "DeltaH=-393.4 KJ "mol"^(-1) The enthalpy change for the transition C_("diamond")rarr C_("graphite") will be :

C (diamond) + O _(2) (g) to CO _(2 (g)) , Delta H =- 398 kJ C _(("graphicle")) +O _(2 (g)) to CO _(2 (g)) , Delta H =- 395 kJ the heat liberated when 1g diamond is converted to 1g graphite is