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The heat of transition (Delta H(t)) of g...

The heat of transition `(Delta H_(t))` of graphite into diamond would be, where
C (graphite) `+O_(2)(g)to CO_(2)(g) , Delta H =` x kJ
C (diamond) `+O_(2)(g)to CO_(2)(g) , Delta H =` y kJ

A

`x_(1) + x_(2)`

B

`x_(2) - x_(1)`

C

`x_(1) - x_(2)`

D

`x_(1)x_(2)`

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The correct Answer is:
B
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One gram mole of graphite and diamond were burnt to form CO_(2) gas: C_(("graphite"))+O_(2)(g)toCO_(2)(g)," "DeltaH^(@)=-399.5kJ C_(("diamond"))+O_(2)(g)toCO_(2)(g)," "DeltaH^(@)=-395.4 kJ

Calculate the DeltaH in joules for C("graphite")toC("diamond") from the following data: C("graphite")+O_(2)(g)toCO_(2)(g):" "DeltaH^(@)=-393.5kJ C("diamond")+O_(2)(g)toCO_(2)(g)," "DeltaH^(@)=-395.4kJ

Calculate the enthalpy of combustion of glucose from the follwoing data : C("graphite") +O_(2)(g) to CO_(2)(g) Delta_(r)H^(@) = -395.0 kJ H_(2)(g) + 1/2 O_(2)(g) to H_(2)O(l) Delta_(r)H^(@) = - 269.4 kJ 6C("graphite") + 6H_(2)(g) + 3O_(2)(g) to C_(6)H_(12)O_(6)(s) Delta_(r)H^(@) = -1169.9 kJ

Calculate the heat of combustion (in KJ) of methane from the following data (i) C ("graphite")+2H_(2)(g) rarr CH_(4) (g), DeltaH=-74.8 kJ (ii) C ("graphite")+O_(2) (g) rarr CO_(2) (g), DeltaH=-393.5 kJ (iii) H_(2(g))+1//2O_(2(g)) rarr H_(2)O_((l)), DeltaH=-286.2 kJ .

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