I need help in doing homeworkCan someone please check my work. **Chemical Equilibrium: Data Sheet****Experiment Table:**| Test Tube | Substance Added /Temperature Change | Color Trial 1 | Color Trial 2 | Equilibrium Shifted Towards | Equilibrium Shifted Towards ||-----------|------------------------------------|-----------------|---------------|-----------------------------|-----------------------------|| 1 | 10 drops water | Reference color | | Reference | Reference || 2 | 8 drops Fe(NO₃)₃ | Dark Red | Dark Red | Forward Reaction | Forward Reaction || 3 | 8 drops KSCN | Dark Red | Dark Red | Forward Reaction | Forward Reaction || 4 | 8 drops HCl | Light Orange | Light Orange | Backward Reaction | Backward Reaction || 5 | 10 drops H₂O + Heat | Light Orange | Light Orange | Forward Reaction | Forward Reaction || 6 | 10 drops H₂O + Cold | Dark Red | Dark Orange | Forward Reaction | Forward Reaction |**Questions:**1. **Show Calculations for Making the 0.01 M Solutions of Fe(NO₃)₃ and KSCN:** - **Fe(NO₃)₃ Calculation:** \[ M_1V_1 = M_2V_2 \] \[ 1.0 \times V_1 = 0.01 \times 50 \] \[ V_1 = 0.5 \, \text{mL} \, \, \text{Fe(NO₃)₃} \] - **KSCN Calculation:** \[ M_1V_1 = M_2V_2 \] \[ 1.0 \times V_1 = 0.01 \times 50 \] \[ V_1 = 0.5 \, \text{mL} \, \, \text{KSCN} \] 2. **Based on Test Tubes 5 and 6, is the Forward Reaction of the Equilibrium Exothermic or Endothermic?** **Hint **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, then 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)

Hello. There are multiple questions posted. The first part has been solved. To receive solutions for the remaining parts, please resubmit the whole question and mention the parts to be solved.In the reaction considered, the solution is mostly yellow when the system contains mostly reactants. The color changes to red when the equilibrium shifts towards products. The observations in the color of the solution upon different changes brought to the system have been tabulated.The addition of Fe(NO3)3 or KSCN increases the concentration of reactants, hence the forward reaction is favored. Upon the addition of HCl, some Fe3+ ions form FeCl4- in the solution. This reduces the concentration of Fe3+ ions. Hence, the backward reaction is favored. That is why the solution has a light orange/yellow color. Upon the addition of heat, the solution displays a light orange/yellow color. The backward reaction occurs resulting in the formation of reactants. The forward reaction is exothermic. In a cold environment, the solution becomes red. This indicates that the backward reaction occurs. Test tube Substrate added/Temperature change Colour trial 1 Colour trial 2 Equilibrium shifted towards Equilibrium shifted towards 1 10 drops water reference - - - 2 8 drops Fe(NO3)3 Dark red Dark red Forward reaction Forward reaction 3 8 drops KSCN Dark red Dark red Forward reaction Forward reaction 4 8 drops HCl Light orange Light orange Backward reaction Backward reaction 5 10 drops H2O + heat Light orange Light orange Backward reaction Backward reaction 6 10 drops H2O + cold. Dark red Dark orange-red Forward reaction Forward reaction From the calculations worked out, M1= 1.0 M and V2=50 mL. 50 mL of 0.1 M solution of Fe(NO3)3 and 50 mL of 0.1 M solution of KSCN is to be prepared from 1.0 M solution of the respective compounds. Taking 0.5 mL from 1.0 M of Fe(NO3)3 and 1.0 M KSCN solution and diluting each to 50 mL, will provide 0.01 M solutions of the reactants. M1V1=M2V2M1=1.0M2=0.01 MV2=50 mLV1=0.01×501.0=0.5 mL