Explain the observation made when chlorine gas is bubbled into asolution of iron (ii) sulphate
Ayellow solution is formed. This is because chlorine oxidizes iron (ii) ions to iron (iii) ions there4 changing the colour of solution from pale green to yellow.
Except I would write it as iron(II) and iron(III)
Those should be Roman numerals.
Sounds OK to me.
Well, when chlorine gas is bubbled into a solution of iron (II) sulfate, you'll see some interesting things happen. It's like a little chemical circus!
First off, the chlorine gas will start to react with the iron (II) sulfate. This reaction is a bit of a balancing act, as chlorine loves to steal electrons from other atoms. So the chlorine gas will snatch away some electrons from the iron ions in the iron (II) sulfate.
As a result, the iron ions are transformed into iron (III) ions. It's like they put on a magic show and changed their number of electrons. Ta-da!
But that's not all! As the chlorine gas continues to react, it will also form a compound called iron (III) chloride. This compound is a bit of a joker, as it's a bright yellow color. So your solution will go from looking boring and colorless to having a vibrant yellow tint. Talk about adding some excitement to the mix!
Overall, the observation you'll make is that the chlorine gas will cause the iron (II) sulfate solution to change color and form iron (III) ions and iron (III) chloride. It's like watching a chemistry acrobat perform. Just don't forget your popcorn!
When chlorine gas is bubbled into a solution of iron (II) sulphate, a series of observations can be made.
1. Color change: Initially, the solution of iron (II) sulphate is pale green in color. However, when chlorine gas is bubbled into the solution, it undergoes a color change to a yellowish-green or yellow-brown color. This indicates the formation of a new compound.
2. Formation of a precipitate: As chlorine gas reacts with iron (II) sulphate, a brownish precipitate forms in the solution. This solid is known as iron (III) hydroxide, which is an insoluble compound. It can be observed as suspended particles in the solution.
The chemical equation for the reaction between chlorine gas and iron (II) sulphate is as follows:
2 FeSO4 + Cl2 -> Fe2(SO4)3 + 2 HCl
To explain how this observation is made, here's the step-by-step approach:
1. Identify the reactants: In this case, the reactants are chlorine gas (Cl2) and iron (II) sulphate (FeSO4).
2. Determine the products: By examining the equation, you can see that the products are iron (III) sulphate (Fe2(SO4)3) and hydrochloric acid (HCl).
3. Understand the reaction: The reaction involves the displacement of iron (II) ions (Fe2+) in the iron (II) sulphate by chlorine gas. This results in the formation of iron (III) sulphate and the release of hydrochloric acid.
4. Analyze the observations: The color change from pale green to yellow-green or yellow-brown indicates the formation of a new compound. The formation of a brownish precipitate, iron (III) hydroxide, suggests the production of an insoluble compound.
By following these steps and understanding the reaction, you can explain the observations obtained when chlorine gas is bubbled into a solution of iron (II) sulphate.