Question

Ammonia is manufactured from nitrogen and hydrogen by the Haber process.
N2(g) + 3H2(g) + 2NH3(9)
What is the percentage yield when 60 kg of ammonia is produced from 60 kg of hydrogen?
A 5.9%
B. 17.6%
С 35.3%
D 50.0%

Answer 1

Answer:

Expected yeild in balanced reaction = 34 * 10 = 340 kg .

But , yeild given = 60 kg

, so percentage yield = ( 60 / 340 ) * 100 = 17.6% .

Hence , option - ( B ) is correct

Answer 2

Given: In Haber process, 60Kg of ammonia, and 60 Kg of hydrogen.

To find The percentage yield of ammonia.

Solution:

In Haber's process, the equation is -

N₂(g) + 3H₂(g) + 2NH₃(g)

According to the law of conservation of mass, one mole of nitrogen reacts with three moles of hydrogen produces two moles of ammonia.

Percentage yield = (Actual yield/theoretical yield) x 100

We know the actual yield of ammonia (60kg) so we need to work out the theoretical yield.

moels of hydrogen = mass of hydrogen taken/molecular mass of hydrogen = 60,000/2 = 30,000 moles.

3:2 ratio of hydrogen and ammonia, so (30,000/3) x 2 = 20,000 mols of Ammonia.

Therefore, mass of ammonia = mr x mols = 20,000 x 17 = 340,000 grams

So percentage yield is (60,000/340,000) x 100 = 17.6

Therefore, the percentage yield of ammonia, when 60 kg of ammonia is produced from 60 kg of hydrogen?is 17.6%