Question

The Haber process is used to make ammonia, which is an important source of nitrogen that can be metabolized by plants. Using the equation below, determine how many kilograms of ammonia will be formed from 89.5 kg of hydrogen. N2(g) + 3H2(g) → 2NH3(g)

Answer 1

Answer:

506kg

Explanation:

From the reaction equation, we can see that 3 moles of hydrogen yielded 2 moles of ammonia.

Now we need to calculate the number of moles of hydrogen reacted. This mathematically equals the mass of hydrogen reacted divided by the molecular mass of the hydrogen molecule.

The mass of hydrogen reacted is 89.5kg. This equals 89.5 × 1000g which equals 89500g. The molecular mass of hydrogen is 2g/mole ( 1 atom of hydrogen has an atomic mass unit of 1 and 1 molecule of hydrogen has 2 atoms).

Now we mathematically calculate the number of moles of hydrogen reacted to be 89500/2 which equals 44,750 moles.

If 3 moles of hydrogen yielded 2 moles of ammonia gas, then 44, 750 moles will yield 44,750 × (2/3) which equals 29,833 moles of Ammonia gas.

Now, let's calculate the mass of Ammonia gas yielded. This mathematically equals the number of moles of ammonia gas yielded multiplied by the molar mass of ammonia gas. The molar mass of ammonia gas is (14 + 3(1)) which equals 17g/mole.

Hence, the mass yielded equals 29,833 × 17 = 506167g

This equals 506,167 ÷ 1000 = 506.167kg.