Type the correct answer in the box. Express the answer to two significant figures Given: [ mathrm(N)_(2)+3 mathrm(H)_(2) arrow 2 mathrm(NH)_(3) ] Bond & }(c) Bond Energy (mathrm(kJ) / mathrm(mol)) mathrm(N)=mathrm(N) & 942 mathrm(H)-mathrm(H) & 432 mathrm(N)-mathrm(H) & 386 Use the bond energies to calculate the change in enthalpy for the reaction. The enthalpy change for the reaction is kilojoules.

To calculate the change in enthalpy ( ) for the given reaction, we will follow these steps:1. Calculate the total energy required to break the bonds in the reactants.2. Calculate the total energy released when the bonds in the products are formed.3. Use the relationship .Given reaction: From the table, we have the following bond energies:- : 942 kJ/mol- : 432 kJ/mol- : 386 kJ/molNow, let's calculate the energy required to break the bonds in the reactants:- For , we have one bond, so the energy required is kJ/mol.- For , we have three bonds, so the energy required is kJ/mol.Total energy required to break the bonds in the reactants: Next, let's calculate the energy released when the bonds in the products are formed:- For , we have six bonds (each has three bonds), so the energy released is kJ/mol.Total energy released when new bonds form: Now, we apply the relationship for : The negative sign indicates that the reaction is exothermic, meaning it releases heat.Therefore, the enthalpy change for the reaction is **-78 kilojoules** when expressed to two significant figures.