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)^(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 H_(2)O_(2) rarr H_(2)O+1/2 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

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 :

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)

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)

The standard enthalpies of formation of H_(2)O_(2(l)) and H_(2)O_((l)) are -187.8kJ "mole"^(-1) and -285.8 kJ "mole"^(-1) respectively. The DeltaH^(0) for the decomposition of one mole of H_(2)O_(2(l)) " to" H_(2)O_((l)) and O_(2(g)) is