Question

Amonia, NH3, is an important industrial chemicial. It is produced using the Haber process from nitrogen, N2, and hydrogen, H2. How much ammonia can be produced from 28kg of nitrogen and 2kg of hydrogen , assuming the reaction yield is 90% A. 10,2 kg B.17.0 kg C. 9.95 kg D. 11.3 kg E. 34.0 kg

* I already put 11.3kg and it says that it was wrong

Answer 1

Molar mass of N2 = 28 g/mol

mass of N2 = 28 kg = 28000 g

we have below equation to be used:

number of mol of N2,

n = mass of N2/molar mass of N2

=(28000 g)/(28 g/mol)

= 1000 mol

Molar mass of H2 = 2 g/mol

mass of H2 = 2 Kg = 2000 g

we have below equation to be used:

number of mol of H2,

n = mass of H2/molar mass of H2

=(2000 g)/(2 g/mol)

= 10000 mol

we have the Balanced chemical equation as:

N2 + 3 H2 ---> 2 NH3

1 mol of N2 reacts with 3 mol of H2

for 1000 mol of N2, 3000 mol of H2 is required

But we have 1000 mol of H2

so, H2 is limiting reagent

we will use H2 in further calculation

Molar mass of NH3 = 17 g/mol

From balanced chemical reaction, we see that

when 3 mol of H2 reacts, 2 mol of NH3 is formed

mol of NH3 formed = (2/3)* moles of H2

= (2/3)*1000

= 666.7 mol

we have below equation to be used:

mass of NH3 = number of mol * molar mass

= 666.7*16

= 11300 g

= 11.3 Kg

% yield = actual mass*100/theoretical mass

90= actual mass*100/11.3

actual mass=10.2 Kg

Answer: A