Ammonia, NH3, and oxygen can be reacted together in the presence of a catalyst to form only nitrogen monoxide and water. The number of moles of oxygen consumed for every 15.0 moles of NO produced is:.

18.75 moles of O2.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

NH3 + O2 —> NO + H2O

There are 3 atoms of H on the left side and 2 atoms on the right side. It can be balance by putting 4 in front of NH3 and 6 in front of H2O as shown below:

4NH3 + O2 —> NO + 6H2O

There are 4 atoms of N on the left side and 1 atom on the right side. It can be balance by putting 4 in front of NO as shown below:

4NH3 + O2 —> 4NO + 6H2O

Now, there are a total of 10 atoms of O on the right side and 2 atoms on the left side. It can be balance by putting 5 in front of O2 as shown below:

4NH3 + 5O2 —> 4NO + 6H2O

Now the equation is balanced.

Now, we can determine the number of moles of oxygen consumed for every 15.0 moles of NO produced as follow:

4NH3 + 5O2 —> 4NO + 6H2O

From the balanced equation above,

5 moles of O2 were consumed to produce 4 moles of NO.

Therefore, Xmol of O2 will be consume to produce 15 moles of NO i.e

Xmol of O2 = (5 x 15)/4

Xmol of O2 = 18.75 moles.

Therefore, 18.75 moles of O2 is consumed for every 15 moles of NO produced.

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