Question

If 80g of x combines with 1.5 * 10^23 atoms of y to form x2y wuthout any of either element remaining .What is the atomic weight of x

Answer 1

Answer:

The atomic weight of x is 160.58 g/mol.

Explanation:

Number of atoms of y =$1.5\times 10^{23} atoms$

Molecular formula of the compound = $x_2y$

2 x atoms are bonded with 1 atom of y.

1 x atom binds with = $\frac{1}{2}y$

Number of atoms required to bind with $1.5\times 10^{23} atoms$ of y:

$1.5\times 10^{23} atoms\times 2=3.0\times 10^{23} atoms$ of x.

Number atoms of x = Moles × $N_A$

$3.0\times 10^{23}=\frac{80 g}{M}\times 6.022\times 10^{23} mol^{-1}$

M = 160.58 g/mol

The atomic weight of x is 160.58 g/mol.

Answer 2

Explanation:

X2Y expresses molar ratio

i.e Y=1.5 × 10 ^23 atoms

              So X = 2(1.5 × 10^23)

Therefore When mass of X is 80 gm .

No. Of atoms is =3 × 10^23 atoms

Gram atomic weight is the weight 1 mole of X (1 mole = 6 × 10^23 atoms)

By cross multiplication u will get atomic at as 160 grams