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Balancing Redox Equations

Calculate the...

Question

Calculate the maximum amount of $B a_{3} (P O_{4})_{2}$ that will form by the reaction of 1 mol of $B a C l_{2}$ with 0.4 mol of $N a_{3} P O_{4}$

A

0.8 mol

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B

0.5 mol

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C

0.2 mol

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D

1 mol

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Solution

The correct option is C 0.2 mol
The balanced chemical reaction of $B a C l_{2}$ with $2 N a_{3} P O_{4}$ is
$3 B a C l_{2} + 2 N a_{3} P O_{4} \to B a_{3} (P O_{4})_{2} ↓ + 6 N a C l$
The mol of $B a C l_{2}$ used is $\frac{3}{2}$ times the mol of $N a_{3} P O_{4}$
$∴$ To react with 0.4 mol of $N a_{3} P O_{4}$ required mol of $B a C l_{2}$ would be $0.4 \times \frac{3}{2} = 0.6$
By 2 mol of $B a C l_{2},$ 1 mol of $B a_{3} (P O_{4})_{2}$ is formed.

Therefore, by $0.4$ mol of $N a_{3} P O_{4 -} = 0.4 \times \frac{1}{2} = 0.2$ mol of $B a_{3} (P O_{4})_{2}$ is formed.

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Balancing Redox Equations

Standard XIII Chemistry

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