For the allotropic change represented by equation \[C(diamond)\to C(graphite)\]; the enthalpy change is \[\Delta H=-1.89\,kJ\]. If \[6\,g\] of diamond and \[6\,g\] of graphite are separately burnt to yield carbon dioxide, the heat liberated in the first case is [KCET 1988; DPMT 2000]

Less than in the second case by \[1.89\,kJ\]

More than in the second case by \[1.89\,kJ\]

Less than in the second case by \[11.34\,kJ\]

More than in the second case by \[0.945\,kJ\]

For the allotropic change represented by equation \[C(diamond)\to C(gr

1.	For the allotropic change represented by equation \[C(diamond)\to C(graphite)\]; the enthalpy change is \[\Delta H=-1.89\,kJ\]. If \[6\,g\] of diamond and \[6\,g\] of graphite are separately burnt to yield carbon dioxide, the heat liberated in the first case is [KCET 1988; DPMT 2000]
A.	Less than in the second case by \[1.89\,kJ\]
B.	More than in the second case by \[1.89\,kJ\]
C.	Less than in the second case by \[11.34\,kJ\]
D.	More than in the second case by \[0.945\,kJ\]
Answer» E.

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For the allotropic change represented by equation \[C(diamond)\to C(graphite)\]; the enthalpy change is \[\Delta H=-1.89\,kJ\]. If \[6\,g\] of diamond and \[6\,g\] of graphite are separately burnt to yield carbon dioxide, the heat liberated in the first case is [KCET 1988; DPMT 2000]

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