Question

Limiting Reactant:

Answer 1

Zn as a limiting reactant

N₂ as an excess reactant

Theoretical Yield : 13.15 g

Further explanation

Reaction

3 Zn + N₂ ⇒ Zn₃N₂

Ar Zn : 65,38 g/mol

Ar N₂ : 28.0134 g/mol

mol Zn

$\tt \dfrac{11.5}{65.38}=0.176$

mol N₂

$\tt \dfrac{9.55}{28.0134}=0.341$

limiting reactant : the smaller ratio(mol:coefficient)

mol ratio Zn : N₂ :

$\tt \dfrac{0.176}{3}\div \dfrac{0341}{1}=0.0586\div 0.341$

Zn as a limiting reactant(smaller ratio)

N₂ as an excess reactant

mol Zn₃N₂ :

$\tt \dfrac{1}{3}\times 0.176=0.0586$

mass of Zn₃N₂ (Theoretical Yield) :

$\tt 0.0586\times 224.154~g/mol=13.15~g$