Calculate the change in enthalpy for thefollowing reaction, using the bond enthalpydata provided below.(note: you may roundthe bond energies to the nearest 100kj·mol−1during your calculations)2n2h2(g) + 3o2(g)←→4no(g) + 2h2o(g)bondbond energy (kj·mol−1)

There are missing information in the question. The bonds enthalpy are:

N=N: 409 kJ/mol

N-H: 388 kJ/mol

O=O: 498 kJ/mol

N=O: 630 kJ/mol

O-H: 463 kJ/mol

+508 kJ/mol

Explanation:

The formation of a bond is endothermic, so the enthalpy is positive, and the break is exothermic, so the enthalpy is negative. The enthalpy of the reactants must be negative, thus, the change in enthalpy can be calculated as:

ΔH = ∑n*H products - ∑n*H reactants, where n is the number of bonds.

N₂H₂ has 1 N=N bond and 2 N-H bonds; O₂ has 1 O=O bond; NO has 1 N=O bond; and H₂O has 2 O-H bonds, so:

ΔH = (4*1*630 + 2*2*463) - [2*(1*409 + 2*388) + 3*1*498)

ΔH = +508 kJ/mol

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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