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zavuch27 [327]
3 years ago
6

If 125.0g of nitrogen is reacted with 125.0g of hydrogen, what is the theoretical yield of the reaction? What is the excess reac

tant? What is the limiting reactant? Show your work.
Chemistry
1 answer:
vaieri [72.5K]3 years ago
8 0

The theoretical yield of the reaction : 151.64 g

The limiting reactant :  N₂

The excess reactant : H₂

<h3>Further explanation</h3>

Reaction

N₂+3H₂⇒2NH₃

A method that can be used to find limiting reactants is to divide the number of moles of known substances by their respective coefficients(mol ratio), and the smaller become a limiting reactant

mass of N₂=125 g

mol N₂(MW=28 g/mol) :

\tt mol=\dfrac{mass}{MW}\\\\mol=\dfrac{125}{28}=4.46

mass H₂ = 125 g

mol H₂(MW= 2 g/mol) :

\tt mol=\dfrac{125}{2}=62.5

From the equation, mol ratio N₂ : H₂ = 1 : 3

Limiting reactant : N₂ : H₂ =

\tt \dfrac{4.46}{1}\div \dfrac{62.5}{3}=4.46\div 20.8

N₂  : limiting reactant

H₂ : excess reactant

mol NH₃ based on limiting(N₂) (from equation N₂ : NH₃ = 1 : 2)

\tt mol~NH_3=\dfrac{2}{1}\times 4.46=8.92

mass NH₃ (MW=17 g/mol) :

\tt mass=mol\times MW\\\\mass=8.92\times 17=151.64

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