An ionic compound mx3 is prepared according to the following unbalanced chemical equation. m + x2 gives mx3, a 0.105-g sample of x2 contains 8.92 x 10^20 molecules. the compound mx3 consists of 54.47% x by mass. what are the identities of m and x, and what is the correct name for mx3? starting with 1.00 g each of m and x2, what mass of mx3 can be prepared?

Atomic mass of 35.5 g/mol is of chlorine.

Atomic mass of 89.02 g/mol is of Yttrium.

Ytterium(III) chloride is the correct name for .

1.835 grams of can be prepared.

Explanation:

Moles of =n

Number of moleules of

1 mole =

n = 0.001481 mole

Mass of

Molar mass of

m = 71 g/mol

Atomic mass of X =

Atomic mass of 35.5 g/mol is of chlorine.

The compound MX3 consists of 54.47% X by mass:

Molar mass of compound = M'

Percentage of element in compound :

X:

M' = 195.52 g/mol

Molar mass of compound = M'

M' = 1 × (atomic mass of M)+ 3 × (atomic mass of X)

195.52 g/mol = atomic mass of M + 3 × (35.5 g/mol)

Atomic mass of M = 89.02 g/mol

Atomic mass of 89.02 g/mol is of Yttrium.

Ytterium(III) chloride is the correct name for .

Moles of Yttrium =

Moles of chlorine gas=

According to reaction, 3 moles of chlorine reacts with 2 moles of Y.

Then 0.01408 moles of chlorine gas will :

of Y.

This means that chlorine is in limiting amount., So, amount of yttrium (III) chloride will depend upon amount of chlorine gas.

According to reaction , 3 moles of chlorine gives 2 moles of

Then 0.01408 moles of chlorine will give :

of

Mass of 0.009387 moles of :

0.009387 mol × 195.52 g/mol = 1.835 g

1.835 grams of can be prepared.

28528289 29823282 8298232 39858