I need help with my homework **Chemical Equilibrium: Data Sheet****Instructions:** Fill in the following table.| Test Tube | Substance Added / Temperature Change | Reference Color | Color Trial 1 | Color Trial 2 | Equilibrium Shifted Towards ||-----------|------------------------------------|-----------------|---------------|---------------|-------------------------------|| 1 | 10 drops water | Dark Red | Reference | | Reference || 2 | 8 drops Fe(CN)3 | Dark Red | Dark Red | | || 3 | 8 drops KSCN | Dark Red | Dark Red | | || 4 | 8 drops HCl | Light Orange | Light Orange | | |Note: The table includes test tube numbers, substances added, reference colors, observations of color changes during trials, and whether the equilibrium shifted. **Chemical Equilibrium****Objective**To observe and explain equilibrium shifts based on Le Chatelier’s Principle.**Introduction**In any chemical reaction, reactants are converted to products. In some cases, some of the products are converted back to reactants. Such reactions are called reversible reactions where reactants are converted to products (forward reaction) and products are converted back to reactants (reverse reaction). When the rate of the forward reaction becomes equal to the rate of the reverse reaction, we say that the reaction is at equilibrium. At this point, there is no change in the concentration of the reactants and the products.We can disturb a reaction at equilibrium by changing the concentration, pressure/volume, or temperature. Le Chatelier’s Principle states that a reaction (system) at equilibrium will stay at equilibrium until acted upon by some outside force that changes the equilibrium conditions—for example, by adding a greater concentration of one of the products or reactants. The system will then adjust to return to equilibrium by counteracting the change that has just been made.Some examples of stresses and how the equilibrium system responds to counteract those stresses are as follows:**Change in Concentration**- If we add a reactant, the equilibrium will shift towards the products. This is because a portion of the added reactant will be used up to form more products until the equilibrium is re-established.- If we remove a reactant, then to compensate for the loss of the reactants, the product will decompose to form reactants and therefore the equilibrium will shift towards the reactants.- If we add a product, the equilibrium will shift to the reactants in order to consume the excess product.- If we remove a product, then to compensate for the loss of the products, more product will be formed from the reactants and the equilibrium will also shift towards the products.**Changes in Temperature**- An endothermic process will be favored (shifting towards the formation of products) by an increase in temperature. The reaction shifts in the direction that absorbs heat to counteract the increase in temperature.- An exothermic process will be favored (shifting towards the formation of products) by a decrease in temperature. The reaction shifts in the direction that releases heat to counteract the decrease in temperature.During this lab, you will investigate Le Chatelier’s Principle using iron(III)-thiocyanate equilibrium. You will be combining Fe(NO₃)₃, (iron

It is given that the aim is to study the reaction and observe the direction of the reaction when the equilibrium reaction is disturbed with the help of Le Chatelier’s principle. The reaction taking place is as follows, 1) Reaction of Fe(NO3)3 and KSCN to produce FeSCN2+, Fe3+(aq) (Yellow) + SCN-(aq) (colorless) ⇌ FeSCN2+(aq) (Red) ; Main Reaction 2) Reaction of HCl and Fe3+ ions from the above reaction to produce FeCl4-, this is a side reaction and disturbing the equilibrium of this reaction disturbs the first reaction as well, Fe3+(aq) (Yellow) + Cl-(aq) (colorless) ⇌ FeCl4-(aq) (colorless) ; Side Reactiona) In the first observation 8 drops of Fe(NO3)3 is added this disturbs the equilibrium of the first reaction and according to the le- chatelier’s principle, the reaction will tend to attain equilibrium again. Thus, the reaction will move in the forward direction as the reactant concentration has been increased and the reaction will tend to decrease the concentration of reactants by moving forward. Thus, for both the trials in observation 1 the reaction will move in the forward direction showing a dark red color. b) In the second observation 8 drops of KSCN is added this disturbs the equilibrium of the first reaction and according to the le-chatelier’s principle, the reaction will tend to attain equilibrium again. Thus, the reaction will move in the forward direction as the reactant concentration has been increased and the reaction will tend to decrease the concentration of reactants by moving forward. Thus, for both the trials in observation 2 the reaction will move in the forward direction showing a dark red color.c) In the third observation 8 drops of HCl is added this disturbs the equilibrium of the first and the second reactions and according to the le- chatelier’s principle the reactions will tend to attain equilibrium again. Thus, the reaction will move in the forward direction in case of the first reaction as the reactant concentration has been increased and the reaction will tend to decrease the concentration of reactants by moving forward. But in the case of the first reaction as the Fe3+ ions is used up by the second reaction. Thus, the reaction will move in the backward direction in case of the first reaction as the reactant concentration has been decreased and the reaction will tend to increase the concentration of reactants by moving backwards. Thus, for both the trials in observation 3 the reaction will move in the backward direction showing a light-orange color.

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Chemical Equilibrium: Data Sheet Name Fill in the following table: Substance Test added Equilibrium shifted towards Color Trial 2 Equilibrium shifted Color Trial 1 tube Temperature change towards Reference Reference Reference color: 1o drops water 1 8 drops Fe CNO3)2 Dark Red DaK Red. 8 drops Dork Red Dark Red 3 KSCN 8 drops Light Light 4. Oronge Oronge HCI