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Identify the limiting reactant when 65.14g of CaCl, reacts with 74.68 g of N to produce CaCO, and NaCl.

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This is an incomplete question, here is a complete question.

Identify the limiting reactant when 65.14 g of CaCl₂, reacts with 74.68 g of Na₂CO₃ to produce CaCO₃, and NaCl.

Answer: The limiting reactant is,
CaCl_2

Explanation : Given,

Mass of
CaCl_2 = 65.14 g

Mass of
Na_2CO_3 = 74.68 g

Molar mass of
CaCl_2 = 111 g/mol

Molar mass of
Na_2CO_3 = 106 g/mol

First we have to calculate the moles of
CaCl_2 and
Na_2CO_3.


\text{Moles of }CaCl_2=\frac{\text{Given mass }CaCl_2}{\text{Molar mass }CaCl_2}


\text{Moles of }CaCl_2=(65.14g)/(111g/mol)=0.587mol

and,


\text{Moles of }Na_2CO_3=\frac{\text{Given mass }Na_2CO_3}{\text{Molar mass }Na_2CO_3}


\text{Moles of }Na_2CO_3=(74.68g)/(106g/mol)=0.704mol

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:


CaCl_2+Na_2CO_3\rightarrow CaCO_3+2NaCl

From the balanced reaction we conclude that

As, 1 mole of
CaCl_2 react with 1 mole of
Na_2CO_3

So, 0.587 mole of
CaCl_2 react with 0.587 mole of
Na_2CO_3

From this we conclude that,
Na_2CO_3 is an excess reagent because the given moles are greater than the required moles and
CaCl_2 is a limiting reagent and it limits the formation of product.

Hence, the limiting reactant is,
CaCl_2

User Hunter S
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