Question

The molar mass of M(OH)2, formed by the hypothetical metal M, is 199.416 g/mol. What is the molar mass of the corresponding sulfide?
Assume that the charge of the metal doesn't change.
Provide your answer in decimal notation rounded to two decimal digits (i.e. to the hundredths place).

Answer 1

Answer:

197.48 g/mol

Explanation:

We must first discover the relative atomic mass of M;

From;

M + 2[ 16 + 1 ] = 199.416

M + 34 = 199.416

M = 199.416 - 34

M= 165.416

Since the sulphide is MS

molar mass = 165.416 + 32.065

molar mass= 197.48 g/mol

Answer 2

The molar mass of the corresponding sulfide is  197.48 g/mol

Calculation of molar mass:

Since The molar mass of M(OH)2, formed by the hypothetical metal M, is 199.416 g/mol.

Now the atomic mass of M should be

M + 2[ 16 + 1 ] = 199.416

M + 34 = 199.416

M = 199.416 - 34

M= 165.416

Since the sulphide is MS

So,

molar mass = 165.416 + 32.065

molar mass= 197.48 g/mol

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