ammonia, NH3 is an important industrial chemical. it is produced using the haber process from nitrogen, N2 and hydrogen, H2. how much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%

mass of ammonia = 10.090 kg

Explanation:

We have the following chemical reaction:

N₂ + 3 H₂ → 2 NH₃

number of moles = mass / molecular weight

number of moles of N₂ = 28 / 14 = 2 kmoles

number of moles of H₂ = 2 / 2 = 1 kmole

We see that the limiting reactant is hydrogen (H₂).

Now we devise the following reasoning:

if 3 kmoles of hydrogen produces 2 kmoles of ammonia

then 1 kmole of hydrogen produces X kmoles of ammonia

X = (1 * 2) / 3 = 0.66 kmoles of ammonia

But the yield is 90% so the real quantity of ammonia produced is:

(90/100) * 0.66 = 0.594 kmoles of ammonia

mass = number of moles * molecular weight

mass of ammonia = 0.594 * 17 = 10.090 kg