Clorine was bubbled through aqueous iron 2 sulphate solution.State what was observed, the ionic equation and name the oxidzing agent.

If you did this you should certainly know what you observed.

I don,t know but need the answers to the question

To determine what was observed, the ionic equation, and the oxidizing agent, we need to understand the reaction that occurs when chlorine is bubbled through aqueous iron(II) sulfate solution.

First, let's write down the balanced chemical equation for the reaction:
Cl2(g) + FeSO4(aq) → FeCl2(aq) + SO2(g)

Here's the breakdown of the reaction:

1. Observations:
When chlorine gas (Cl2) is bubbled through the aqueous iron(II) sulfate solution (FeSO4(aq)), the following observations can be made:
- The solution turns from colorless to pale green as iron forms a complex with chlorine.
- Bubbles of gas may be observed, which is sulfur dioxide (SO2) gas.

2. Ionic Equation:
The ionic equation represents the reaction in terms of individual ions. In this case, since all the reactants and products are soluble, we can write the ionic equation as follows:
Cl2 + Fe2+ + SO42- → 2Cl- + Fe2+ + SO42-

3. Oxidizing Agent:
The oxidizing agent is the substance that undergoes reduction during the reaction. It gains electrons, causing another substance to be oxidized. In this reaction, chlorine (Cl2) gains two electrons to form chloride ions (Cl-), indicating that it has been reduced. Therefore, chlorine is the oxidizing agent.

To summarize:
- Observations: Pale green color in the solution and the release of sulfur dioxide gas.
- Ionic Equation: Cl2 + Fe2+ + SO42- → 2Cl- + Fe2+ + SO42-
- Oxidizing Agent: Chlorine (Cl2) is the oxidizing agent.