Heat of formation of `H_(2)O` is -188kJ/mol and `H_(2)O_(2)` is -286 kJ/mol. The enthalpy change for the reaction,
`2H_(2)O_(2) to 2H_(2)O+O_(2)`

If DeltaH_(f)^(@) for H_(2)O_(2) and H_(2)O are -188 kJ/mole and -286 kJ/mole, what will be the enthalpy change of the reaction H_(2)O_(2) rarr H_(2)O+1/2 O_(2)

If DeltaH_(f)^(@) for H_(2)O_(2)(l) and H_(2)O(l) are -188kJ and mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2)(l)to2H_(2)O(l)+O_(2)(g) ?

If DeltaH_f^@" for " H_2O and H_2O_2 " are " -280 and -188 kJ mol^(-1) , the enthalpy change for the reaction, 2 H_2O_2 (l) to 2H_2O (l) + O_2(g) is :

If DeltaH_(f)^(0) " for" H_(2)O_(2(l)) and H_(2)O_((l)) " are " -188 kJ mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2(l)) rarr 2H_(2)O_((l)) + O_(2(g)) = ?

If DeltaH_(f)^(@) for H_(2)O_(2) and H_(2)O are -188 kJ/mole and -286 kJ/mole, what will be the enthalpy change of the reaction