For which one of the following reactions is δh°rxn equal to the heat of formation of the product? for which one of the following reactions is h°rxn equal to the heat of formation of the product? (1/2)a. n2 (g) + o2 (g) → no2(g) b. p (g) + 4h (g) + br (g) → ph4br (l)c. 12c (g) + 11h2 (g) + 11o (g) → c6h22o11 (g) d. n2 (g) + 3h2 (g) → 2nh3 (g) e. 6c (s) + 6h (g) → c6h6 (l)

The reaction in which ΔH°rxn is equal to the heat of formation of the product is 1/2N2 (g) + O2 (g) → NO2(g)

The standard enthalpy change for a reaction is obtained as the difference between the enthalpy change of the reactants and the products. It is a state function hence it depends on the initial and final states of the system.

Note that the standard enthalpy change for a reaction is calculated from the formula;

ΔH°rxn = [n∑(ΔH°products - n∑(ΔH°reactants]

For the reaction; 1/2N2 (g) + O2 (g) → NO2(g), the ΔH°reactants = zero because they are in standard state therefore, ΔH°rxn is equal to the heat of formation of the product.

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atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8