Thermochemistry. Answer, step by step please. (show work)

Question

1N2 (g) + 3H2 (g) = 2NH3 (g) ∆H = -91.2 kJ

a. Is this exothermic or endothermic?

b. Rewrite the equation with the energy as either a reactant or a product.

c. What quantity of heat is released when 41.0 L of Ammonia is produced?

Answer 1

N₂ (g) + 3H₂ (g) = 2NH₃ (g) ∆H = -91.2 kJ

a. Since the sign of ∆H is negative, it is EXOTHERMIC

b. N₂ (g) + 3H₂ (g) = 2NH₃ (g) + heat

c. 41.0 L NH3 x -91.2 kJ / 2 L NH3 = 1870 L