Question

The equivalent weight of a divalent metal is $31.82$ . The weight of a single atom is (in g):

• A. $32.55/$$(6.02$$\times {10}^{23})$
• B. $32.77/$$(6.02$$\times {10}^{23})$
• C. $63.64$
• D. $63.64/$$(6.02$$\times {10}^{23})$

Answer 1

The correct option is D $63.64/$$(6.02$$\times {10}^{23})$

Equivalent weight $=\frac{Molecularweight}{Valency}$

Thus, molecular weight $=31.82\times 2=63.64$

$63.64$ g of metal contains $6.023\times {10}^{23}$ atoms of it.

$\therefore 1$ atom weighs $\frac{63.64}{6.02\times {10}^{23}}$ g.

Hence, option D is correct.