CHEMISTRY PROBLEM! NEED HELP AND WORK SHOWN!

Question

Ammonia can be produced through the Haber process shown in the chemical reaction below. The reaction is known to have a percent yield of 55.1% because it is an equilibrium reaction. How much of each reactant (in grams) will you need yo start with if you want to obtain 200kg of ammonia?

Chemical Equation:

N^2 + 3H^2 >> 2NH^3

Please show work, I don’t understand how to do this problem.

Answer 1

Write out the balanced chemical equation:

N₂ + 3H₂ → 2NH₃

Now, percent yield is as follows:

Percent Yield = (Actual Yield/Theoretical Yield) x 100%

Thus, theoretical yield is:

Theoretical Yield = (Actual Yield/Percent Yield) x 100% (or, we can simply remove the percentage by moving our decimal point two places to the left, the math comes out the same)

The process is the same as usual for stoichiometry problems, but in this case, you must also multiply by the theoretical yield correction to take into account the 55.1% yield (thus, for our answers, they would be GREATER than what we would normally calculate without the correction):

200 kg NH₃ x (1000 g NH₃/1 kg NH₃) x (1 mol NH₃/17 g NH₃) x (1 mol N₂/2 mol NH₃) x (28 g N₂/1 mol N₂) x (1/0.551) =

2.99 x 10⁵ g N₂

200 kg NH₃ x (1000 g NH₃/1 kg NH₃) x (1 mol NH₃/17 g NH₃) x (3 mol H₂/2 mol NH₃) x (2 g H₂/1 mol H₂) x(1/0.551) =

6.41 x 10⁴ g H₂