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A chemist dissolves 10.0 g of MgCl2 (95.21 g/mol) and 10.0 g of Na3PO4 (163.94 g/mol) into water. The product Mg3(PO4)2 (262.87 g/mol) is insoluble in water and crashes out of solution as a white solid. Assuming the reaction goes to completion, how many grams of Mg3(PO4)2 are produced? (Hint: balance the reaction below and identify the limiting reagent) MgCl2(aq) + Na3P04(aq) → NaCl(aq) + Mg3(PO4)2(s)

User Reyno
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1 Answer

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Answer : The mass of
Mg_3(PO_4)_2 produced are 5.3 grams.

Solution : Given,

Mass of
MgCl_2 = 10.0 g

Mass of
Na_3PO_4 = 10.0 g

Molar mass of
MgCl_2 = 95.21 g/mole

Molar mass of
Na_3PO_4 = 163.94 g/mole

Molar mass of
Mg_3(PO_4)_2 = 262.87 g/mole

First we have to calculate the moles of
MgCl_2 and
Na_3PO_4.


\text{ Moles of }MgCl_2=\frac{\text{ Mass of }MgCl_2}{\text{ Molar mass of }MgCl_2}=(10.0g)/(95.21g/mole)=0.105moles


\text{ Moles of }Na_3PO_4=\frac{\text{ Mass of }Na_3PO_4}{\text{ Molar mass of }Na_3PO_4}=(10.0g)/(163.94g/mole)=0.060moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction will be,


2MgCl_2(aq)+3Na_3PO_4(aq)\rightarrow 6NaCl(aq)+Mg_3(PO_4)_2(s)

From the balanced reaction we conclude that

As, 3 mole of
Na_3PO_4 react with 2 mole of
MgCl_2

So, 0.060 moles of
Na_3PO_4 react with
0.060* (2)/(3)=0.040 moles of
MgCl_2

From this we conclude that,
MgCl_2 is an excess reagent because the given moles are greater than the required moles and
Na_3PO_4 is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of
Mg_3(PO_4)_2

From the reaction, we conclude that

As, 3 mole of
Na_3PO_4 react to give 1 mole of
Mg_3(PO_4)_2

So, 0.06 moles of
Na_3PO_4 react to give
(0.060)/(3)=0.020 moles of
Mg_3(PO_4)_2

Now we have to calculate the mass of
Mg_3(PO_4)_2


\text{ Mass of }Mg_3(PO_4)_2=\text{ Moles of }Mg_3(PO_4)_2* \text{ Molar mass of }Mg_3(PO_4)_2


\text{ Mass of }Mg_3(PO_4)_2=(0.020moles)* (262.87g/mole)=5.3g

Therefore, the mass of
Mg_3(PO_4)_2 produced are 5.3 grams.

User Istvano
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