If the standard formation- enthalpy of `CS_(2) , CO_(2)` and `SO_(2)` are `117 kJ * mol^(-1) , -393 kJ * mol^(-1)` and `-297 kJ * mol^(-1)` respectively , calculate the standard reaction enthalpy of - `CS_(2) + 3O_(2) to CO_(2) + 2 SO_(2)`

If the standard formation enthalpy of CS_2, CO_2 and SO_2 are 117 kJ mol^(-1) -393 kJ mol^(-1) and -297 kJ mol^(-1) respectively then calculate the standard reaction enthalpy of the reaction- CS_2 + 30_2 rarr CO_2 2SO_3 .

At 25^(@)C and 1 atm, heat of formation of C_(2)H_(4) (g), CO_(2)(g) and H_(2)O(l) are 52 " kJ mol"^(-1), -394 " kJ mol"^(-1) and -286 " kJ mol"^(-1) respectively. Calculate the heat of combustion of C_(2)H_(4)(g) .

Al(s) and Fe(s) are oxidised by oxygen to form Al_(2)O_(3)(s) and Fe_(2)O_(3)(s) respectively. If the standard enthalpy of formation of Al_(2)O_(3)(s) and Fe_(2)O_(3)(s) are -1669.8 " kJ mol"^(-1) and -824.2 " kJ mol"^(-1) respectively, calculate the change in enthalpy of the given reaction : 2Al(s)+Fe_(2)O_(3)(s) to 2Fe(s)+Al_(2)O_(3)(s)

At 25^(@)C temperature, the standard heat of formation of CH_(4)(g),CO_(2)(g) and H_(2)O(g) are -74.8 kJ*mol^(-1),-393.5kJ*mol^(-1)&-241.6kJ*mol^(-1) respectively. How much heat will be evolved during combustion of 1m^(3)CH_(4)(g) at 25^(@)C temperature and 1 atm pressure ? Consider CH_(4)(g) behaves like an ideal gas.

The enthalpy of combustion of methane, graphite and dihydrogen at 298K are -890.3 kJ*mol^(-1) , -393.5 kJ*mol^(-1) and -285.8kJ*mol^(-1) respectively. Enthalpy of formation of CH_(4)(g) will be-

The standard enthalpies of formation of CO_2(g), H_2O(l) and glucose (s) at 25^@C are -400 kJ/mol, -300 kJ/mol and -1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25^@C Is

The standard bond dissociation energy of A_(2)(g),B_(2)(g) and AB(g) molecules are x, y and z kJ*mol^(-1) respectively. What will be the standard enthalpy of formation of AB(g)?

Enthalpies of formation of CO(g), CO_2(g),N_2O(g) and N_2O_4(g) are -110,-393,81 and 9.7KJ mol^(-1) respectively calculate Delta H_r for the reaction : N_2O_4(g)+3CO(g)rarr N_2O(g)+3CO_2(g)

The heat of reaction for the following reaction (DeltaH^(0)) at 25^(@)C temperatue is -1368 kJ: C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l) If the enthalpy of formation of CO_(2)(g) and H_(2)O(l) at 25^(@)C are -393.5 and -285.8 kJ*mol^(-1) respectively, then what will be the value of the standard enthalpy of formation of C_(2)H_(5)OH(l) ?