Question

3CaCl2 + 2K3PO4 Ca3(PO4)2 + 6KCl
How many moles of potassium phosphate are needed to produce 0.076 mole of potassium
chloride?
ANWERS FAST PLZ

Answer 1

Answer:

ans is 0.25 mole..........

Answer 2

Answer:  $0.0253$ moles of potassium phosphate are required to produce $0.076$ moles of potassium chloride.

Explanation:

The given reaction is between Calcium chloride and potassium phosphate which forms calcium phosphate and potassium chloride as products:

$3 CaCl_{2} + 2 K_{3} PO_{4}$  →  $Ca_{3} (PO_{4} )_{2} + 6 KCl$

Now this reaction indicates that $2$ moles of potassium phosphate $(K_{3} PO_{4})$ are needed to produce $6$ moles of potassium chloride $(KCl)$.

Or $6$ moles of $KCl$ are produced by $= 2$ mole of $K_{3} PO_{4}$

∴ $1$ mole of $KCl$ is produced by  $=\frac{2}{6}$ moles of $K_{3} PO_{4}$

$0.076$ moles of $KCl$ are  produced by  $= \frac{2}{6} * 0.076$ moles of $K_{3} PO_{4}$

                                                                   $= 0.0253$ moles of $K_{3} PO_{4}$

It means $0.0253$ moles of $K_{3} PO_{4}$ are needed to produce $0.076$ moles of $KCl$.

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