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 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 ?

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

The standard heat of combustion of graphite carbon is -393.5 kJ mol^(-1) . The standard enthalpy of CO_(2) is

If the standard molar enthalpy change for combustion of graphite powder is -2.48 xx 10^(2)kJ mol^(-1) , the amount of heat generated on combustion of 1g of graphite powder is ______kJ. (Nearest integer).

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 carbon and carbon monoxide are -393.5 and -283 kJ mol^(-1) respectively. The enthaly of formation of carbon monoxide per mole is :

The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283 kJ mol^(-1) respectively. The enthaly of formation of carbon monoxide per mole is :

The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283 kJ mol^(-1) respectively. The enthaly of formation of carbon monoxide per mole is :

The heat of formation of CO_(2) is -393kj mol^(-1). The amount of heat evoled in the dormation of 0.156 kg of CO_(2) is