If the enthalpy of combustion of diamond and graphite are `-395.4 kJ mol^(-1)` and `-393.6 kJ mol^(-1)`, what is enthalpy change for the `C("graphite") rarr C("diamond")`?

If the enthalpy of combustion of diamond and graphite are -395.4kJ mol^(-1) and -393.6 kJ mol^(-1) what is the enthalpy change for the C (graphite) rarr C (diamond) conversion ?

The enthalpies of combustion of diamond and graphite are - 395.4 kJ and - 393.5 kJ respectively calculate the enthalpy of transformation from diamond to graphite.

The enthalpies of combustion of diamond and graphite are - 395.4 kJ and - 393.5 kJ respectively calculate the enthalpy of transformation from diamond to graphite.

If the enthalpy of combustion of C (graphite) is -393.3kJ mol^(-1) , then for producing 39.3kJ of heat the amount of carbon required is

If the enthalpy of combustion of C (graphite) is -393.3kJ mol^(-1) , then for producing 39.3kJ of heat the amount of carbon required is

What will be the enthalpy change of conversion of graphite into diamond

The enthalpy of combustion of graphite and diamond are -393.5 kJ and -395 kJ respectively. Which of them is more stable ?

The enthalpies of combustion of C_(("graphite")) and C_(("diamond")) are -393.5 and -395.4kJ//mol respectively. The enthalpy of conversion of C_(("graphite")) to C_(("diamond")) in kJ/mol is: