Question

Sulfur reacts with ammonia to give a product A that contains 69.6% by mass sulfur and 30.4% by mass nitrogen and has a molar mass of 184.3 g.

The S and N atoms in the product A alternate around a ring, with half of the atoms having formal charges. Draw two possible electron-dot structures for A.

Answer 1

S + NH3 --> A (69.6% S, 30.4% N) MW = 184.3 g

Calculate mass of S:

m of S = x*MW specie = 0.696*184.3 = 128.2728 g

Calculate mass of N

m of N = y*MW specie = 0.304*184.3 = 56.0272 g

Ratio S:N = 128.2728 /56.0272 = 2.28947

First, identify

MW of S = 32 G/mol

MW NH3 = 17 g/mol

MW of N = 14 g/mol

S:N ratio:

1:1 = 1 mol of S:1 mol of N = 32/14 = 2.28571

Then,

the ratio is:

1:1

SN

Empirical formul --> SN

Total formula:

n = MW/empirical MW = 184.3 / (14+32) = 4.00652

S4N4