Alferid Hussin ShifaCHM (Course 124) (Section 01)Lab (4) Oct 3/2019Lab 4: Chemical Reaction “Can Go Forward and Backward”Objective: In this experiment, we are attempting to observe how chemical reactions can be reversibleSpecially, we will investigate the factors that can disturb an equilibrium system. List of chemicals, & hazard:- Sodium Hydroxide - NaOH- Hydrochloric Acid - HCl- Calcium Chloride - CaC l2- Ethanol (easily flammable) - C2H6O- Iron (III) - Thiocyanate- AcetoneList of Chemicals with Safety Hazard: There are Hazards chemicals in this experiment.I. Safety Precautions:- Be cation when handling the acidic solutionII. Waste Disposal:- Disposal the mixtures in the sink, or into the appropriate waste beaker.List of Equipment:Test tubes Pipet aid & disposable pipet’s (Three of 10 mL)Beaker Tube rackDistilled water Graduated cylindersHot water bath & ice bath Pre-Lab Questions:NoneProcedure in short: 1. Obtain a test tube rack, containing 6 small test tubes. 2. Prepare a hot and ice water bath, each in beakers. 3. Set up an observation table with each system having its own row. 4. Mix the solution according to each system present on the table.5. Following each system, observe the direction of shift that the reaction followed. 6. Repeat this process if needed.ResultSystem 1System/Tube # Disturbance Observed Change Direction of Shift11 Control Orange/Red -2 Iron Dark red →3 Potassium Dark red →4 Sodium Hydroxide Light red ←5 Hot bath Light red ←6 Ice bath Dark red→System 2System/Tube # Disturbance Observed Change Direction of Shift1 Control Green -2 Hydrochloric Acid yellow ←3 Sodium Hydroxide Blue →System 3System/Tube # Disturbance Observed Change Direction of Shift1-1 Control Green -1-2 Calcium Chloride Dark Green →1-3 Ethanol Light Green ←1-4 Hot Bath Light Green ←1-5 Ice Bath Dark Green →System 4System/Tube # Disturbance Observed Change Direction of Shift1 Control Red -2 Calcium Chloride Dark Purple →3 Acetone Purple →4 Hot bath Dark Purple →5Ice bathLight red ←2Post lab 1)No visible changes can be observed when a system is at equilibrium because the rate of the forward reaction equals the rate of the backward reaction. Hence the concentration of reactants and products remains constant over time causing no visible change.2)a) Increasing the concentration of a reactant will make the reaction moves towards right (product side) and more products are formed.b) Decreasing the concentration of a reactant will the reaction moves towards left (reactant side) and more reactants are formed.c) Increasing the temperature of the system will make the rate increase.d) Decreasing the temperature of the system will make the rate decrease.3)The rates of both forward and backward reactions do not equal immediately after an equilibrium system is disturbed.4)a) If the rate of the forward reaction is increased, the direction of shift would be towards theforward direction.b) If the rate of the reverse reaction is increased, the direction of shift would be towards the reverse direction.c) If the rate of the forward reaction was decreased, the direction of shift would be towards the reverse direction.d) If the rate of the reverse reaction was decreased, the direction of shift would be towards the forward direction.5.The shift of equilibrium systems will be towards the direction with the higher rate of reaction.6. a. Forward reaction.b. Reverse reaction.c. Reverse reaction.d. Forward reaction.e. Reverse reaction.f. Forward reaction.g. Forward reaction.h. Reverse reaction.Any specific observations:- No specific observations were madeConclusion:- The overall point of this experiment was to display the reversibility of the specific reactions that we were given. Throughout this experiment we had proven that all are indeed a reversive reaction. Also, we proven that factors such as heat, concentration can alter the equilibrium in the direction of the product or reacted depending on the