Question

One gram metal ion M2+ was discharged by the passage of 1.81 ×10^22 electrons . What is the atomic weight of metal

Answer 1

Moles of electrons that were being discharged are => 1.81*10^23/(6*10^23) = > 0.301 moles.

Atomic weight = > moles / weight => 0.301/1=> 0.301 g

Answer 2

The atomic weight of metal is 66.5 g/mol

Explanation:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains $6.022\times 10^{23}$ number of particles.

We know that:

Charge on 1 electron = $1.6\times 10^{-19}C$

Charge on 1 mole of electrons = $1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C$

Let atomic weight is x.

$M\rightarrow M^{2+}+2e^-$

x gram of $M^{2+}$ is discharged by $2\times 6.022\times 10^{23}$

electrons

1 g of $M^{2+}$ is discharged by $\frac{12.04\times 10^{23}}{x}\times 1=1.81\times 10^{22}$

electrons

x =66.5 g/mol

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