Two reactions are given below :
`C_("(graphite)")+O_(2(g))rarrCO_(2(g)),DeltaH=-393.7kJ`
`C_("(diamond)")rarrC_("(graphite)"),DeltaH=-2.1kJ`
What quantity of diamond will give 800 kJ of heat on burning ?

Given that: i. C("graphite") +O_(2)(g) rarr CO_(2)(g), DeltaH =- 393.7 kJ ii. C("diamond") rarr C("graphite"), DeltaH =- 2.1 kJ a. Calculate DeltaH for buring of diamond of CO_(2) . b. Calculate the quantity of graphite that must be burnt to evolve 5000 kJ of heta.

Given that: i. C("graphite") +O_(2)(g) rarr CO_(2)(g), DeltaH =- 393.7 kJ ii. C("diamond") rarr C("graphite"), DeltaH =- 2.1 kJ a. Calculate DeltaH for buring of diamond of CO_(2) . b. Calculate the quantity of graphite that must be burnt to evolve 5000 kJ of heta.

For the transition C_("(diamond)") rarr C_("(graphite)"), DeltaH=-1.5 kJ . It follows that

For the transition C_("(diamond)") rarr C_("(graphite)"), DeltaH=-1.5 kJ . It follows that

C_("graphite")+O_(2)(g)rarrCO_(2)(g) deltaH=-94.05Kcalmol^(-1) C_("diamond")+O_(2)(g),DeltaH=-94.50Kcalmol^(-1) Therefore,

Given : C("diamond")+O_(2)rarrCO_(2),DeltaH=-395 kJ C("graphite")+O_(2)rarrCO_(2),DeltaH=-393 kJ The enthalpy of formation of diamond from graphite is