The heat of combustion of C(graphite) and CO(g) are` -390 kJ//"mole and " -280 kJ//"mole"` respectively.
`CO(g)+Cl_(2)(g)to COCl_(2)(g)Delta H=+208 kJ`
Calculate heat of formation `("in kJ"//"mole")` of `COCl_(2)(g)` (in kJ/mole)

The heats of formation of CO_(2(g)) and H_(2)O_((l)) are - 398 and -285 kJ mol^(-1) respectively. The heat of combustton of methane is -390 kJ. The heat of formation of methane will be

C(s)+(1)/(2)O_(2)(g)to CO(g), Delta H =- 42 kJ/mole CO(g)+(1)/(2)O_(2)(g)to CO_(2)(g) , Delta H =-24 kJ/mole The heat of formation of CO_(2) is

C(s)+(1)/(2)O_(2)(g)to CO(g), Delta H =- 42 kJ/mole CO(g)+(1)/(2)O_(2)(g)to CO_(2)(g) , Delta H =-24 kJ/mole The heat of formation of CO_(2) is

Heat change for a reaction N_(2)(g) + 3H_(2) (g) to 2NH_(3)(g) is - 92.2 kj/mol. Calculate the heat of formation of one mole of a ammonia.

The equations representing the combustion of carbon and carbon monoxide are : C(s) + O_(2)(g) to CO_(2)(g) DeltaH = -394 (kJ)/(mol) CO(s) + 1/2 O_(2)(g) to CO_(2)(g) DeltaH = -284.5 (kJ)/(mol) the heat of formation of 1 mol of CO(g) is :

Molar enthalpy of combustion of C_(2)H_(2)(g),C_("graphite")andH_(2)(g) are -1300,-394, and -286 KJ/mole respectively , then , Calculate Bond enthalpy of C-=C bond inKJ /mole: "Given" : DeltaH_("sub") (C_("graphite"))=715 KJ//"mole" DeltaH_(BE)(H-H)=436 KJ//"mole" DeltaH_(BE)(C-H)=413KJ//"mole"

From the following data , C_("s , graphite") + O_(2(g)) to CO_(2 (g)) Delta H^(@) = - 393 . 5 kJ /mole H_(2) (g) + 1//2 O_(2) (g) to H_(2)O (l) Delta H^(@) = -286 kJ/mole 2C_(2) H_(6) (g) + 7O_(2) (g) to 4 CO_(2 (g)) + 6H_(2)O (l) Delta H^(@) = - 3120 kJ/mole Calculate the standard enthalpy of formation of C_(2) H_(6) (g) (in kJ/mole)