Final answer:
The question appears to contain a mismatch between the reaction description and the provided heats of formation values. None of the options correctly calculate the heat of reaction for the formation of ammonia. The provided heat of formation values relate to a different reaction, and hence, an accurate answer cannot be deduced without the correct data.
Step-by-step explanation:
To calculate the standard heat of reaction for the formation of ammonia from hydrogen gas and oxygen gas, we must use Hess's law and the standard heats of formation (ΔH°f) for the substances involved in the reaction. The correct mathematical representation considering the standard heat of formation values provided should reflect the enthalpy change for the reaction using the formula ΔH° = ΣΔH°f(products) − ΣΔH°f(reactants). In this case, however, there seems to be some confusion in the provided options, as the reaction described involves the formation of ammonia (NH3), but the heats of formation are for a different compound. Nonetheless, for a hypothetical reaction forming NH3, the valid math statement using the provided numbers would match choice (b), but with the correct substances involved. The process would look like: 2(heat of formation of NH3) - [3(ΔH°f of H2 which is 0) + ΔH°f of O2 (also 0)] = ΔH°. In conclusion, without the correct values for the formation of ammonia, a valid math claim cannot be established with the given options.