INTRODUCTIONChemical equilibrium represents a balance between the forward and reverse reactions. Changes in experimental conditions can disturb the balance and shift the equilibrium so that more or less product is formed. Conditions that can change the experimental conditions are: Change in concentration Change in pressure Change in volume Change in temperatureLe Ch$$teliers principle helps predict the direction $($forward or back$)$ a reaction will shift when an external stress $($change in concentration, pressure, volume, or temperature$)$ is applied to a system in equilibrium.In this experiment we will be using the reaction:Fe$3+($aq$)+$ SCN$-($aq$)$ FeSCN$2+($aq$)$ Equation $1$We will study the response of this system to various stresses and explain these results in terms of Le Ch$$teliers Principle.PROCEDUREInto a clean $600$ mL beaker add $250$ mL deionized water, $1$ mL of $1$ M KSCN and $1$ mL of $1$ M Fe$($NO$3)3$ solution. This is the stock solution and can be shared between two groups. The stock solution will have an intense red color due to the formation of the complex FeSCN$2+.$ Obtain $9$ clean medium sized test tubes and label $1-9.$ Add $10$ mL of the stock solution into each test tube. Test Tube $1$ is the control. Add the following reagents to test tubes $2-8.$Table $1.$ Test tube preparationTest TubeReagent added and amount$1$No reagent added, this is the control$22$ mL of $1$ M Fe$($NO$3)331$ mL of $1$ M KSCN$40\mathrm{.}5$ mL $($or $10$ drops$)$ of $0\mathrm{.}1$ M AgNO$3($Note: this can stain your skin$)52$ mL of $12$ M HCl$61$ mL of $1$ M Na$3$PO$471$ mL of $0\mathrm{.}1$ M Na$2$C$2$O$48$Several crystals of NaF$9$No reagent added. Heat test tube $9$ in a hot water bath Cover each test tube with parafilm and mix. Compare the color intensity of test tubes $2-9$ with the control, test tube $1.$ Record observations in terms of Le Ch$$teliers principle. The darkest test tube will have a higher concentration of FeSCN$2+.$Use Table $2$ to explain your observations and write the net ionic equations for the post lab.Table $2.$ Complexes and Precipitates Ag$+$Cl$-$PO$43-$F$-$C$2$O$42-$Fe$3+$ FeCl$4-$FePO$4($s$)$FeF$63-$Fe$($C$2$O$4)3-$SCN$-$AgSCN $($s$)$ DisposalDispose of all chemicals in the waste container in the hood. $1$ Le Ch$$teliers Principle in Iron Thiocyanate Equilibrium OBSERVATIONS$/$DATATest Tube NumberReagent AddedObservationExplanation$123456789$ Heat added $1$ Le Ch$$teliers Principle in Iron Thiocyanate Equilibrium POSTLAB$1.$ Write the equilibrium constant expression $($K$=)$ for the reaction between Fe$3+$ and SCN$-.2.$ Based on your observation in test tube $9,$ is the reaction between Fe$3+$ and SCN$-$ exothermic or endothermic? $3.$ Write the net ionic equations of any reaction that occurred in test tubes $4-8.($use Table $2).$