What is the molar enthalpy of formation for ammonia?
Hi I'm having issues relating hess's law to this question:
The given chemical equation represent the combustion of ammonia and the combustion of hydrogen 1. 4NH3+3O2-->6H2O + 2N2. ( deltaH1 = -1516 kJ) 2. 2H2+O2 --> H2O ( deltaH2 = -572 kJ) What is the molar enthalpy of formation for ammonia? A. -100kJ B.-50kJ C. 50KJ D.100KJ
I'm not sure how I would apply the product - reactant equation here or rearrange the equation to get my answer since I don't have an initial reaction to compare it to. How would I go about answering this question?