The first step in the ostwald process for producing nitric acid is as follows: 4nh3(g) + 5o2(g) ? 4no(g) + 6h2o(g). if the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

4 moles of NH3 reacts with 5 moles of O2.
4 moles of NH3 = 4 (14 + 3*1) = 68g
5 moles of O2 = 5*32 = 160g
Therefore, 68g of NH3 reacts with 160g of O2
Mass of NH3 to react with 15g of oxygen = 15*68 / 160 = 6.375g, which is less than 15 g.
Mass of O2 to react with 15g of NH3 = 15*160 / 68 = 35.29g, which is more than 15g. 
Therefore, the limiting reactant is O2, which means the reaction will proceed until the 15 g of oxygen finish.

4 moles of NO = 4 (14+16) 120g
Therefore, 160g of O2 gives 120g of NO.
15g of O2 will give Xg of NO.
X (theoritical yeild) = 15*120 / 160 = 11.25g
Practical yield = 8.70g
Yield = practical yeild / theoritical yeild *100 = 8.70/11.25 = 77.33%

Adozen is 1221/12 = 1.751.75 x 12 = 21therefore, 1.75 is the answer.