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For the following reaction, {:(C("diam...

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:

A

1.59kcal

B

0.1375 kcal

C

0.55kcal

D

0.275kcal

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The correct Answer is:
d
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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:

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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

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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 :

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

If C(s)+O_(2)(g)to CO_(2)(g),DeltaH=rand CO(g)+1/2O_(2)to CO_(2)(g),DeltaH=s then, the heat of formation of CO is

C_("diamond")+O_(2)(g)rarrCO_(2)(g),DeltaH=-395 kJ ...... (i) C_("graphite")+O_(2)(g)rarrCO_(2)(g),DeltaH=-393.5KJ" "…(ii) The DeltaH , when diamond is formed from graphite, is

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