Decomposition Of HS-Copper(II) Nitrate For The Synthesis Of Sulfur

This paper outlines the preparation of nitrogen dioxide through nitrate decomposition and is commonly used for the production of sulfur for many smelting processes according to Wikipedia.

They say when it rains, it pours. This is not an entirely accurate saying, but it does make for an appropriate catch phrase that can embody the precious lesson I was able to derive from this technical article in regards to the decomposition of HS-Copper(II) Nitrate for the synthesis of sulfur. Factors such as being oriented and cleaning out your reaction vessel can go a long way towards making your experiments more successful after all!

What is HS-Copper(II) Nitrate?

HS-Copper 2(NO3) Cl is a bright green compound meaning it is easily oxidized. Many copper compounds are colored with copper ions and they all work in the same way. Cu2+ forms an octahedral complex or MXO4. There are many different complexes of copper ions, but in HS-copper II(NO3) cl, there are four nitric acid molecules instead of two. Normally these molecules react to form hydrogen sulfide gas, something that could happen if iron filings were put into potassium alum containing water. With this reaction, the animal actually produces the needed nitrogen gas because naturally occurring nitrates are involved in most nitrogen-fixing reactions done by plants

How to Make HS Copper Nitrate

To produce copper sulfate, copper nitrate is produced and then reacted with sulfur to make the copper sulfite complex. The method of making this complex is done by heating copper nitrate in a hot water solution for about 2 hours.

Zinc and copper nitrate are mixed together in order to carry out the synthesis of sulfur. This reaction is run in a high temperature bath in an inert atmosphere for about 2 hours.

Reaction Mechanism of HS Copper Nitrate

HS-Copper Nitrate reacts with sulfate to form copper sulfate. CuSO4 will eventually be reduced to copper sulfide and H2S gas in a tightly sealed container such as copper sulfite (CuSO3).

The HS-Copper(II) Nitrate is the first step in a two-step hydrolysis of copper sulfate to copper sulfide. 

In the first step, Co3(OH)2.CuSO4 is coprecipitated by acid, and henceforth an equimolar amount of sulfur dioxide and sulfuric acid are produced yielding a 1:1 mole ratio.

In the second step, CuSO4 is further decomposed by liquid ammonia and elemental sulfur obtained by cooling.

What Is The Synthesis Of Sulfur From HS Copper Nitrate

Copper metal is heated in nitric acid at a temperature of 230C/450F under an oxygen-free atmosphere to produce copper oxide and nitrous oxide. The copper oxide, also called copper oxide (CuO) is then reacted with sulfuric acid in the presence of 700-800 atmospheric pressure hydrogen sulfide gas to produce the intermediate product, HS-copper(II) sulfate. At this point, hydrogen sulfide gas decomposes into sulfur dioxide gas which reacts with the HS-copper(II) sulfate to form elemental sulfur particles or droplets that eventually come out as greenish-yellow H 2 S0 4

Blog Outline:

A copper(II) nitrate solution is reduced with hydrochloric acid to copper(I) acetate. If a K2HgO4 solution is slowly added to this copper(I) acetate solution, then it will react to form a multistep synthesis of sulfur.

Copper(II) Nitrate is a reagent that is found easily. The purpose of this lab is to decompose the copper(II) nitrate so we can obtain some of the metallic copper by performing the Sulfur synthesis. 

First, 50mL of water was added to 500g of copper nitrate (Cu(NO 3 ) 2 ). With a beaker underneath it, vigorously shake the copper in the liquid and try to dissolve as much copper as possible. A test solution was made from 1M hydrazine hydrate (NH 2 OH), which would show the particular coloration solution against a pure water counter-rod.

The original citric acid solution has little yellowish precipitate on top due to Cu2+ ions, which pinkish-orange precipitate and purple residues are formed when HCl is added dropwise between all three solutions (to extract K2CO 3 ) implying that Cu2+ ions remain in citric acid.

As a comparative experiment also conducted, without K2CO3 dry chemical being present at room temperature, no pollution happened at first with 500ml 11% NH3H205 being exposed to it in a beaker for 8 seconds, indicating that it takes 8 seconds for

How Sulfur is Headed

Copper(II) Nitrates are important elemental molecules that play a role in the synthesis of sulfur. In this blog, I will discuss how their reactivity can be influenced for the synthesis of sulfur.

Copper(II) nitrate is squirted into water and the sulfuric acid separates from the copper. The water will solidify, leaving us with the copper(II) sulfate. This process is conducted in three steps; separation, precipitation, and oxidation.

Introduce Some Tools You Will Need

The copper, sulfur(II) sodium sulfate, and nitric salt were placed in a tin lined, 3 neck round bottom flask. The copper penny was used to convert the sulfide into copper metal. Once complete- the copper, zinc rod and aluminum wire were added.

Steps in Synthesis

Synthesis of sulfur from copper(II) nitrate gives a good yield and is easy to oxidize with oxygen to obtain elemental sulfur.