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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 $N a_{3} P O_{4}$

0.8 mol

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0.5 mol

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0.2 mol

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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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Similar questions

Q. 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}

If 0.5 mol of $B a C l_{2}$ is mixed with 0.2 mol of $N a_{3} P O_{4}$ , the maximum number of moles of $B a_{3} (P O_{4})_{2}$ that can be formed is:

Q. If 0.5 mol of

B a C l_{2}

is mixed with 0.20 mol of

N a_{3} P O_{4}

, the maximum amount of

B a_{3} (P O_{4})_{2}

that can be formed is :

Q. If 0.5 moles of

B a C l_{2}

is mixed with 0.1 moles of

N a_{3} P O_{4},

the maximum amount of

B a_{3} (P O_{4})_{2}

that can be formed is

3 B a C l_{2} + 2 N a_{2} P O_{4} \to B a_{3} (P O_{4})_{2} + 6 N a C l

Maximum amount of

B a_{3} (P O_{4})_{2}

formed when

2

moles each of

N a_{3} P O_{4}

and

B a C l_{2}

react is:

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Balancing Redox Equations

Standard XII Chemistry

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