an aqueous solution contains 1 mol of S2O3 ions and this reduces 4 mol chlorine molecules.What is the sulphur containing product of this reaction?
To determine the sulfur-containing product of this reaction, we need to recognize the chemical equation representing the reduction of chlorine by thiosulfate ions (S2O3 ions). The balanced equation for this reaction is:
2 S2O3^2- + 4 Cl2 → S4O6^2- + 4 Cl^-
From this equation, we can see that 2 moles of thiosulfate ions (S2O3^2-) react with 4 moles of chlorine molecules (Cl2). This means that if we have 1 mole of thiosulfate ions, we would need 2 moles of chlorine molecules for a complete reaction.
However, in your question, it states that we have 4 moles of chlorine molecules. This means that there is an excess of chlorine available for the reaction. Therefore, the reaction will go to completion, and all the thiosulfate ions will be used.
According to the balanced equation, the sulfur-containing product of this reaction is S4O6^2-. This product is known as tetrathionate ion.
So, tetrathionate ion (S4O6^2-) is the sulfur-containing product of this reaction when an aqueous solution containing 1 mole of S2O3 ions reacts with an excess of chlorine.