A7 When chlorine gas is bubbled through Iron (II) chloride, the following reaction occurs: \[ 2 \mathrm{FeC} \ell_{2(\mathrm{aq})}+\mathrm{C} \ell_{2(\hat{\theta})} \rightarrow 2 \mathrm{FeC} \ell_{3(\mathrm{aq})} \] (a) What colour change is observed in this reaction? \( \qquad \) [1] (b) The above reaction is a redox reaction. State with a reason which substance is reduced. (i) reduced \( \qquad \) (ii) the oxidising agent \( \qquad \) (c) Write an ionic equation for the reaction above. \( \qquad \) \( \qquad \) [Total 7]

### (a) Colour Change Observed When chlorine gas is bubbled through iron(II) chloride solution, the solution changes from **pale green to yellow**. ### (b) Identification of Redox Components **(i) Substance Reduced:** Chlorine (**Cl₂**) is reduced because it gains electrons during the reaction. **(ii) Oxidizing Agent:** Chlorine (**Cl₂**) acts as the oxidizing agent because it accepts electrons from iron(II) chloride, facilitating the oxidation of iron. ### (c) Ionic Equation for the Reaction The net ionic equation for the reaction is: \[ 2\, \mathrm{Fe}^{2+}(\mathrm{aq}) + \mathrm{Cl}_2(\mathrm{g}) \rightarrow 2\, \mathrm{Fe}^{3+}(\mathrm{aq}) + 2\, \mathrm{Cl}^{-}(\mathrm{aq}) \]