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 standard internal change in multiples of -10^(2)KJ 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)), HF_((g)) " are " +20, -250 and -270KJ "mole"^(-1)

Calculate the standard enthalpy change for the reaction CH_4(g) +2O_2(g) rarr CO_2(g)+2H_2O(l) Given that the standard enthalpies of formation of CH_4(g),CO_2(g), and H_2O(l) are -74.8 kJ mol^-1, -393.5 kJ mol^-1 and -285.8 kJ 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), CO_(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 multiplied by its stiochiometric coefficient in the balanced equation, minus the corresponding sum of the standard molar enthalpies of formation of the reactants

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 heat of the following reaction at constant pressure, F_(2)O(g)+H_(2)O(g)rarrO_(2)(g)+2HF(g) The heats of formation of F_(2)O(g),H_(2)O(g) and HF(g) are 5.5 kcal-57kcal and -64 kcal repectively.

Calculate heat of the following reaction at constant pressure, F_(2)O(g)+H_(2)O(g)rarrO_(2)(g)+2HF(g) The heats of formation of F_(2)O(g),H_(2)O(g) and HF(g) are 5.5 kcal-57kcal and -64 kcal repectively.

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.