Question

2.0 g of a metallic carbonate on decomposition gave 1.5g of metallic oxide.the equivalent mass of metal is​

Answer 1

Answer:

Formula used is =$\frac{weight of metal carbonate}{weight of metallic oxide}$

=$\frac{eq.mass of metal+eql.mass of CO_{3} ^{2} }{eq.mass of metal+eq.mass of O^{2} }$

$\frac{2}{x+30} =\frac{1.5}{x+8}$

2(x+8)=1.5(x+30)

2x+16=1.5x+45

0.5x=45-16

x=58

Answer 2

The equivalent mass of metal is​, 58 g.eq

Explanation:

Equivalent weight : It is the molar mass of a substance divided by the number of equivalents in the substance.

Given :

Weight of metallic carbonate = 2.0 g

Weight of metallic oxide  = 1.5 g

First we have to determine the equivalent weight of oxide and carbonate.

Molar mass of $O_2$ = 32 g/mole

$\text{Equivalent weight of }O_2=\frac{\text{Molar mass of }O_2}{\text{Number of valency}}=\frac{32}{4}=8g.eq$

Molar mass of $CO_3^{2-}$ = 60 g/mole

$\text{Equivalent weight of }CO_3^{2-}=\frac{\text{Molar mass of }CO_3^{2-}}{\text{Number of valency}}=\frac{60}{2}=30g.eq$

Let the equivalent weight of metal be x.

Gram equivalent of metallic carbonate = Gram equivalent of metallic oxide

$\frac{\text{Given weight of carbonate}}{\text{Equivalent weight of metal}+\text{Equivalent weight of carbonate}}=\frac{\text{Given weight of oxide}}{\text{Equivalent weight of metal}+\text{Equivalent weight of oxide}}$

Now put all the given values in this expression, we get:

$\frac{2.0}{x+30}=\frac{1.5}{x+8}$

$1.5(x+30)=2(x+8)$

$1.5x+45=2x+16$

$0.5x=29$

$x=58$

Therefore, the equivalent mass of metal is​, 58 g.eq

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