Question

Gaseous ammonia chemically reacts with oxygen gas to produce nitrogen monoxide gas and water vapor. Calculate the moles of oxygen needed to produce 1.6 mol of nitrogen monoxide. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

Answer 1

Answer:

2 mol

Explanation:

4NH3 + 5O2. --> 4NO + 6H2O

you can see that 4 mole of NO is required for 5

mol of O2

so,. 1 mole of NO gives = 5/4

1.6 mole = 5/4 × 1.6

= 2 mol

Answer 2

Answer:

The moles of oxygen needed to produce 1.6 mol of nitrogen monoxide = 2 mol.

Explanation:

• When the gaseous ammonia reacts with the oxygen we obtain nitrogen monoxide and water vapor.
• This reaction is a combustion reaction as well as a red-ox reaction. It is an exothermic process as a large amount of heat is liberated.
• 4NH₃ (g) + 5O₂ (g) → 4NO (g) + 6H₂O (vap)

Calculation:

• In the equation above we can see that 4 moles of NH₃ react with 5 moles of O₂ to produce 4 moles of NO. The mole ratio of O₂:NO is 5:4.

• When we have to produce 1.6 moles of NO, then moles of O₂ needed to be supplied will be:

⇒ $\frac{5}{4}$ × 1.6

⇒ $\frac{8}{4}$

⇒ 2 mol

Conclusion:

2 moles of O₂ produce 1.6 moles of NO.