`4Li(s)+O_(2)(g)to2Li_(2)O(s)`
At `25^(@)C,DeltaH` for this reaction is -598.8 kilo joules per mole of Li should be reacted with excess `O_(2)(g)` in order to relaase 150 Kj?

Fe_(2)O_(2)(s)+(3)/(2)C(s)to(3)/(2)CO_(2)(g)+2Fe(s) DeltaH^(@)=+234.12KJ C(s)+O_(2)(g)toCO_(2)(g) DeltaH^(@)=-393.5KJ Use these equations and DeltaH^(@) value to calculate DeltaH^(@) for this reaction : 4Fe(s)+3O_(2)(g)to2Fe_(2)O_(3)(s)

Fe_(2)O_(2)(s)+(3)/(2)C(s)to(3)/(2)CO_(2)(g)+2Fe(s) DeltaH^(@)=+234.12KJ C(s)+O_(2)(g)toCO_(2)(g) DeltaH^(@)=-393.5KJ Use these equations and DeltaH^(@) value to calculate DeltaH^(@) for this reaction : 4Fe(s)+3O_(2)(g)to2Fe_(2)O_(3)(s)

For the reaction, 2H_(2)(g)+O_(2)(g) to 2H_(2)O(g), DeltaH=-573.2kJ The heat of decomposition of water per mole

For the reaction, 2H_(2)(g)+O_(2)(g) to 2H_(2)O(g), DeltaH=-573.2kJ The heat of decomposition of water per mole

2C_"(s)" + O_(2(g)) to 2CO_((g)) , DeltaH = - 220 KJ, Which statement is correct for the reaction :-

C(s)+(1)/(2)O_(2)(g)toCO(g),DeltaH=-110.4kJ . Does this DeltaH represent enthalpy of combustion of carbon?

Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ Heat of reaction for the reaction, FeO(s) + Fe_(2)O_(3)(s) to Fe_(3)O_(4)(s) is :