Based on the following data, is this iron thiocyanate reaction endothermic or exothermic?: Fe3+(aq) + SCN−(aq) ⇌ FeSCN2+(aq)[colorless] [colorless] [blood-red color]After being submreged in a hot water bath, the solution was colorless.After being submerged in an ice bath, the solution turned dark red in color. ### Chemical Equilibrium Reaction Observation**Chemical Equation:**\[ \text{Fe}^{3+} (aq) + \text{SCN}^- (aq) \leftrightarrows \text{FeSCN}^{2+} (aq) \]*Blood-red color*This reaction demonstrates the concept of chemical equilibrium with a visible color change. Below are the observations from different experimental conditions:#### Table 1. Equilibrium Response Observations| Test Tube | Color Observation | Reaction Response ||-----------|---------------------------|----------------------|| **Test tube 1 - Control** | Light red | Select a response || **Test tube 2 - Add KSCN (aq)** | Slightly darker red | Towards reactants || **Test tube 3 - Add Fe(NO₃) (aq)** | Darker red | Towards reactants || **Test tube 4 - Add NaF (s)** | No color | Towards products || **Test tube 5 - Hot water bath** | Almost colorless | Towards products || **Test tube 6 - Ice bath** | Slightly darker red | Towards reactants |**Details:**- **Test tube 1 (Control):** The solution shows a light red color, serving as the baseline for further tests. - **Test tube 2 (Add KSCN):** Adding potassium thiocyanate results in a slightly darker red color, indicating a shift towards the reactants.- **Test tube 3 (Add Fe(NO₃)):** The addition of iron(III) nitrate darkens the red color further, suggesting a shift towards the reactants as more Fe³⁺ ions are available.- **Test tube 4 (Add NaF):** The solution becomes colorless due to the formation of a complex that consumes Fe³⁺, shifting equilibrium towards the products.- **Test tube 5 (Hot water bath):** Heating the solution makes it almost colorless, indicating a shift towards the products, likely due to increased kinetic energy favoring the reaction in that direction.- **Test tube 6 (Ice bath):** Cooling the solution results in a slightly darker red color, indicating a shift towards the reactants due to decreased kinetic energy.These observations highlight how changes in concentration and temperature can influence the position of equilibrium

The balanced reaction is – Fe3+aq + SCN- aq ⇔FeSCN2+aqcolorless colorless blood red color High temperature Low temperature At high temperatures, the solution is colorless. At low temperatures, the solution is dark red. This shows that the formation of iron thiocyanate leads to the release of heat as energy. So, the reaction is exothermic.