The "Haber" process for producing ammonia is shown as follows:
N₂ (g) + 3 H₂ (g) →2 NH₃ (g) How many liters of gaseous ammonia, NH₃, are produced from 20.0 moles of N₂ gas at 500 ° C and 200 atm?

Question

Quizplus · Accepted Answer

We can use the balanced equation to determine the ratio of moles of nitrogen gas to moles of ammonia gas produced: 1 mole N₂ produces 2 moles NH₃ Therefore, 20.0 moles of N₂ will produce: 20.0 moles N₂ × (2 moles NH₃ / 1 mole N₂) = 40.0 moles NH₃ Next, we can use the ideal gas law to convert moles of ammonia gas to liters at the given conditions: PV = nRT V = nRT/P V = (40.0 mol)(0.0821 L·atm/mol·K)(500 K)/(200 atm) V = 12.7 L Therefore, the answer is choice B, 12.7 L.

The "Haber" Process for Producing Ammonia Is Shown as Follows