Tetraphosphorous decoxide (P₄O₁₀) reacts with water to produce phosphoric acid. Write the balanced equation for this reaction. Do not include states of matter in the equation.

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 Determine the number of moles of P₄O₁₀ required to produce 5.80 moles of phosphoric acid.

  mol

 Determine the number of moles of water required to produce 5.80 moles of phosphoric acid.

  mol 

1) Balanced chemical reaction:

P₄O₁₀+6H₂O --------> 4H₃PO₄

 

2) 1.45 moles of P₄O₁₀ are required to produce 5.80 moles of phosphoric acid

 

3) 8.7 moles of H₂O are required to produce 5.80 moles of phosphoric acid

Step-by-step explanation

1) Balanced chemical equation for the given reaction:

P₄O₁₀+6H₂O ------> 4H₃PO₄

1 mole of tetraphosphorous decoxide (P₄O₁₀) reacts with 6 moles of water to produce 4 moles of phosphoric acid (H₃PO₄)

 

There are basic steps of balancing chemical equation as follows:

 

i) Consider, simple unbalanced equation:

P₄O₁₀+H₂O ------> H₃PO₄

Tetraphosphorous decoxide reacts with water to produce phosphoric acid

 

ii) Count number of atoms of each element on both side in given equation:

On left hand side (reactants):

P= 4 , O= 11, H= 2

On right hand side(product):

P= 1, O= 4, H= 3

 

iii) Balance complex atoms first other than hydrogen and oxygen. Balance the element which is present in single molecule on reactants and product side beside hydrogen and oxygen by adjusting their coefficient.

Here, phosphorus (P) is a single element present in only one molecule on both side. Hence we should balance phosphorus first.

 

iv) Balance phosphorus on both side:

phosphorus atoms on reactant side= 4

phosphorus atoms on product side= 1

Add coefficient 4 to the molecule containing phosphorus on products side to balance with 4P on reactant side.

Hence, by adding coefficient to the molecule on product side we get,

P₄O₁₀+H₂O -----> 4H₃PO₄

Now count the atoms of each element

on both side of reaction,

On left hand side (reactants):

P= 4 , O= 11, H= 2

On right hand side(product):

P= 4, O= 16, H= 12

Hence, Phosphorus is balanced on both side.

 

v) Balance the hydrogen atoms on left hand side by adding coefficient:

Number of H on right hand side= 12 and Number of H on left hand side= 2

Hence, to balance 12 atoms of H on right hand side we can add 6 as a coefficient to H₂O on left hand side to get,

P₄O₁₀+ 6H₂O -----> 4H₃PO₄

Now count the atoms of each element

on both side of reaction,

On left hand side (reactants):

P= 4 , O= 16, H= 12

On right hand side(product):,

P=4, O= 16, H= 12

Hence, hydrogen is balanced on both side.

 

vi) Balance oxygen atoms:

As we can see, all the atoms of each element on both side are balanced (P=4, H=12, O=16) now, no need to further balance oxygen separately. Hence, the reaction is balanced.

 

vii) Write balanced chemical reaction:

P₄O₁₀+ 6H₂O -----> 4H₃PO₄

 

 

2) From balanced equation, If 1 mole of P₄O₁₀ is required for formation of 4 moles of H₃PO₄ then, moles of P₄O₁₀ required for production of 5.80 moles of H₃PO₄ is,

= 5.80×1/4 moles

= 1.45 moles of P₄O₁₀

Hence, 1.45 moles of P₄O₁₀ are required to produce 5.80 moles of phosphoric acid

 

3) From balanced equation, If 6 moles of H₂O (water) is required for formation of 4 moles of H3PO4 then, moles of H₂O required for production of 5.80 moles of H3PO4 is,

= 5.80×6/4 moles

= 8.7 moles of H₂O

Hence, 8.7 moles of H₂O are required to produce 5.80 moles of phosphoric acid