Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6% S and 30.4% N. Measurements of its molecular mass yield a value of 184.3 g/mol. The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length.
(a) Calculate the empirical and molecular formulas for the substance. (b) Write Lewis structures for the molecule, based on the information you are given. (Hint: You should find a relatively small number of dominant Lewis structures.), (c) Predict the bond distances between the atoms in the ring. (Note: The S–S distance in the S8 ring is 2.05 Å.), (d) The enthalpy of formation of the compound is estimated to be 480 kJ/mol-1. ΔHf° of S(g) is 222.8 kJ/mol-1. Estimate the average bond enthalpy in the compound.
We need at least 10 more requests to produce the solution.
0 / 10 have requested this problem solution
The more requests, the faster the answer.