What will be the standard enthalpy change for gaseous reaction `C Cl_4 + 2H_2O rarr CO_2 + 4HCL` if standard heat of formations for `CO_2`(g), `C Cl_4`, HCl(g) and `H_2O`(g) are 393.7, -106.7, -92.5 and -241.8 kJ/mol

Calculate the standard enegry change for the reaction: OF_(2)(g) +H_(2)O(g) rarr O_(2)(g) +2HF(g) at 298K The standard enthalpies of formation of OF_(2)(g), H_(2)O(g) , and HF(g) are +20, -250 , and -270 kJ mol^(-1) , respectively.

Calculate the enthalpy change for the reaction CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) The enethalpy of formation of CH_(4)(g),CO_(2)(g) and H_(2)O(l) are -74.8 kJ mol^(-1) , -393.5 kJ mol^(-1) and -285.8 kJ mol^(-1) respectively.

The combustion of butane (C_(4)H_(10)) is exothermic by 2878.7 kJ "mol"^(-1) .Calculate the standard enthalpy of formation of butane given that the standard enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 kJ "mol"^(-1) and -285.8 kJ "mol"^(-1) respectively.

Calculate Delta_(f)H^(@) for the reaction, CO_(2)(g) + H_(2)(g) to CO(g) + H_(2)O(g) Given that Delta_(f)H^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5, -111.3 and -241.8 kJ mol^(-1) respectively.

Calculate the standard enthalpy of combustion of CH_(4) , it standard enthalpies of formation of CH_(4(g)),H_(2)O_((l)), and CO_(2(g)) are -74.81kJ mol^(-1), -285.83kJ mol^(-1) and -393.51kJ mol^(-1) respectively.

Find the value of Delta_(f) H^(@) for the reaction N_(2) O_(4) (g) + 3 CO(g) rarr N_(2) O (g) + 3 CO_(2) (g) Standard enthalpies of formation of CO(g), CI_(2) (g), N_(2) O (g) , and N_(2) O_(4) (g) are - 110, - 393, 81 , and 9.7 kJ mol^(-1) , respectively. Strategy : The standard enthalpy change of a reaction is equal to the sum of the standard molar enthalpie of formation of the products each miltiplied by its stiochiometric coefficient in the balanced equation, minus the corresponding sum of the standard molar enthalpies of formation of the reactants

Calculate the standard enthalpy of formation of propane (C_(3)H_(8)) if its enthalpy of combustion is -2220.2 kJ "mol"^(-1) .The enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 and -285.8 kJ "mol"^(-1) respectively.

Calculate the standard enthalpy of formation of ethylene, C_(2)H_(4)(g) from the following thermochemical equation : C_(2)H_(4)(g) + 3O_(2)(g) to 2CO_(2)(g) + 2H_(2)O(g) Delta_(r)H^(@) = -1323 kJ Given the standard enthalpy of formation of CO_(2)(g) and H_(2)O(g) are - 393.5 and -249 kJ mol^(-1) respectively.