Nitric oxide, no, is made from the oxidation of nh3, and the reaction is represented by the equation 4nh3 + 5o2 ? 4no + 6h2o an 9.5-g sample of nh3 gives 12.0 g of no. the percent yield of no is :

The percent yield of NO is 71.43 %.

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of ammonia = 9.5 g

Molar mass of ammonia = 17 g/mol

Putting values in equation 1, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

4 moles of ammonia produces 4 moles of NO

So, 0.56 moles of ammonia will produce of NO

Now, calculating the mass of NO from equation 1, we get:

Molar mass of NO = 30 g/mol

Moles of NO = 0.56 moles

Putting values in equation 1, we get:

Experimental yield of NO = 12.0 g

Theoretical yield of NO = 16.8 g

Putting values in above equation, we get:

Hence, the percent yield of NO is 71.43 %.

it's filtration, but this is an assumption so my apologies if i got this