Constants Periodic Table1 1.33 g H2 s altowed to react with 9.82 g N. producing

Question

Constants Periodic Table1 1.33 g H2 s altowed to react with 9.82 g N. producing 2.35 g NH, The Haber- In the Haber-Bosch process, hydrogen gas reacts with nitrogen process to the equation Part A 3H2(g) + N2(g)-+2NH (g) range of uses, from fertilkzer to pharmaceuticals the in lower yields than Express your answer to three significant figures and include the appropriate units those predicted from the chemical equation. View Available Hint(s) Express your answer to three significant figures and include the appropriate units alue Units

Explanation / Answer

A)

Molar mass of H2 = 2.016 g/mol

mass(H2)= 1.33 g

use:

number of mol of H2,

n = mass of H2/molar mass of H2

=(1.33 g)/(2.016 g/mol)

= 0.6597 mol

Molar mass of N2 = 28.02 g/mol

mass(N2)= 9.82 g

use:

number of mol of N2,

n = mass of N2/molar mass of N2

=(9.82 g)/(28.02 g/mol)

= 0.3505 mol

Balanced chemical equation is:

3 H2 + N2 ---> 2 NH3

3 mol of H2 reacts with 1 mol of N2

for 0.6597 mol of H2, 0.2199 mol of N2 is required

But we have 0.3505 mol of N2

so, H2 is limiting reagent

we will use H2 in further calculation

Molar mass of NH3,

MM = 1*MM(N) + 3*MM(H)

= 1*14.01 + 3*1.008

= 17.034 g/mol

According to balanced equation

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

= (2/3)*0.6597

= 0.4398 mol

use:

mass of NH3 = number of mol * molar mass

= 0.4398*17.03

= 7.492 g

Answer: 7.49 g

B)

% yield = actual mass*100/theoretical mass

= 2.35*100/7.492

= 31.4 %

Answer: 31.4 %

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---