Question

N₂ (g) + 3H₂ (g) → 2NH₃(g) ΔH = -92.2 kJ

What mass of ammonia is theoretically produced if the above reaction released 183 kJ of heat?

Please show work

Answer 1

One mole of nitrogen reacts with three moles of hydrogen to form two moles of ammonia and 92.2 kJ of heat is released.

Hence, 92.2 kJ of heat is released in formation of 2 moles of ammonia. Calculate number of moles of ammonia formed when energy released is 183 kJ.

Number of moles of ammonia = (2 moles of ammonia / 92.2 kJ) x 183 kJ of energy

Number of moles of ammonia = 3.97 mol

Therefore, 3.97 moles of ammonia is formed along with release of 183 kJ of heat. Molar mass of ammonia is 17.031 g/mol. Calculate weight of 3.97 moles of ammonia gas.

Weight of 3.97 moles of ammonia = (3.97 mol) x (17.031 g/mol)

Weight of 3.97 moles of ammonia = 67.6 g

Therefore, mass of ammonia theoretically produced during release of 183 kJ of heat is 67.6 g.