What is the energy absorbed or released when 1.0 mole of NO is produced?

Question

2 N2O (g) + O2 (g) ---> 4 NO (G)

+82 +90 (kJ/mol)

Answer 1

2N₂O(g) + O₂(g) ==> 4NO(g) ... balanced equation

You provide values of +82 and +90 kJ/mol, but you don't state what those values are. Are they ∆Hºf? Assuming they are, proceed as follows:

∑∆Hf_products - ∑∆Hf_reactants = ∆Hrxn

(4x90) - (2x82) = 360 - 164 = ∆Hrxn

∆Hrxn = +196 kJ when 2 mol N₂O reacts

∆Hrxn/mole = 196/2 = +98 kJ/mol