Question

Using the Haber-Bosch process...

Answer 1

The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation

3H2(g)+N2(g)→2NH3(g)

The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation.

1.61g H2 is allowed to react with 9.91g N2, producing 1.64g NH3.

What is the theoretical yield for this reaction under the given conditions?

What is the percent yield for this reaction under the given conditions?

Answer 2

1. determine limiting reactant

2. use the moles of limiting reactant to calculate the theoretical yield of product
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Using the stoichiometric coefficients to find moles produced.

e.g. for a general reaction:

\(\color{red}{a}A + \color{blue}{b}B\) \(\rightleftharpoons\) \( \color{green}{c}C\)

where upper case are the species (A,B,C), and lower case (a,b,c) are the coefficients (in red),

\(\dfrac{n_A}{\color{red}{a}}=\dfrac{n_B}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\)


so if you have moles of B= 2, how many moles of C did you produce?

solve algebraically: \(\dfrac{2}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\rightarrow n_c=\dfrac{2*\color{green}{c}}{\color{blue}{b}}\)

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"What is the percent yield for this reaction under the given conditions?"

percent yield= \(\dfrac{actual\;yield}{theoretical\;yield}*100\%\)