if 15 g of nitrogen reacts with 15 g of hydrogen, 10.5 g of ammonia is produced. what is the percent yeild of this reaction?

Answer 1

This is a limiting reagent and a percent yield problem rolled into one. I know it is limiting reagent because amounts are given for BOTH reactants.
N2 + 2H2 ==> 2NH3
mols N2 = grams/molar mass
mols H2 = grams/molar mass
Using the coefficients in the balanced equation, convert mols H2 to mols NH3.
Do the same for mols N2 to mols NH3.

It is likely that these two numbers will not be the same which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that number is the limiting reagent. Using the smaller value convert to grams NH3. This is the theoretical yield.
%yield = (actual yield/theo yield)*100 = ?

Answer 2

i need help plz . the question is:if 15 g of nitrogen reacts with 15 g of hydrogen, 10.5 g of ammonia is produced. what is the percent yeild of this reaction?

Answer 3

need help :)