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.

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.