Suppose 1.32 grams of H2 is allowed to react with 10.4 grams of N2, and 1.58 grams of NH3 is...


Suppose 1.32 grams of {eq}H_2 {/eq} is allowed to react with 10.4 grams of {eq}N_2 {/eq}, and 1.58 grams of {eq}NH_3 {/eq} is produced. What is the percent yield for this reaction?

{eq}3H_2(g) + N_2(g) \to 2NH_3(g) {/eq}


Ammonia is a compound having three hydrogen atoms bonded to a nitrogen atom. The nitrogen contains lone pair electrons. It is mainly used as fertilizer and also in the manufacturing of plastics, pesticides, etc.

Answer and Explanation: 1

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The reaction is shown below:

{eq}{\rm{3}}{{\rm{H}}_{\rm{2}}}\left( {\rm{g}} \right) + {{\rm{N}}_{\rm{2}}}\left( {\rm{g}} \right) \to...

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Learn more about this topic:

Calculating Reaction Yield and Percentage Yield from a Limiting Reactant


Chapter 9 / Lesson 6

How to calculate the theoretical yield? Learn the definition and formula of percent yield. Use the theoretical yield equation to calculate theoretical yield.

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