Chemical equilibrium and le chatelier's principle lab answers

Chemical Equilibrium, assignment help
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Science

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I have done an experiment called "Chemical Equilibrium and Le Chatelier’s Principle" . I have collected all needed data. Moreover, I have upload them in here. I need you to read the file called "Chemical Equilibrium and Le Chatelier’s Principle" and do what is exactly asking you for. the Zip file called data is the data that i have collected. The zip file called " exp " is the experiment note if you need to understand something use it. it is just for your extra help.Exp 5. Chemical equilibrium and Le Chatelier’s principle • Exp 3 report is due. • Next class: Exp 6 part ABC only • Chemical equilibrium is achieved when the rates of two opposing chemical reactions become equal. General equilibrium equation aA + bB cC + dD Equilibrium constant: 𝐶 𝐾= 𝐴 𝑐 𝑎 𝐷 𝐵 𝑑 𝑏 K is large, molar concentrations of products > molar concentrations of reactants at equilibrium. K is small, molar concentrations of products < molar concentrations of reactants at equilibrium. Le Chatelier’s principle • A change in factors that determine the equilibrium conditions causes the system to response in a way that counteract the change. • Goal: To study how changes in concentrations (reactants or products), acidity and temperatures affect a chemical equilibrium using observations. Changes in concentration aA + bB cC + dD An increase in reactant concentration (A, B) causes the equilibrium to shift to the right (reducing reactant concentration by forming more products) And vice versa. Changes in acidity are changes in [H+] Changes in temperature • Endothermic reaction: aA + bB + heat cC + dD A temperature increase (heat addition) causes the system to shift to the right (product formation) and vice versa. • Exothermic reaction: aA + bB cC + dD + heat A temperature increase (heat addition) causes the system to shift to the left (reactant formation) and vice versa. Model equilibrium system [Co(H2O)6] 2+ (aq) + 4 Cl- (aq) [Co(H2O)6] 2+ and [CoCl4] 2- [CoCl4] 2- (aq) + 6 H2O (l) have two different colors. By observing the color of the solution, you can deduce how the equilibrium responds to changes. Part A: Determine the color of Co(II) complexes • Which predominant species that reaction 1 and 2 produces? [Co(H2O)6] 2+ or [CoCl4] 2- ? • What is the color? • You will use part A as a reference point for part B! • Check your conclusion of part A with the instructor. Part B: Test tube #1 1. Initial solution: System at equilibrium Prediction: N/A Does the system shift to the left or right? Predict how the color of solution changes Observation: How does the color of the solution change? Do you notice temperature difference? Predominant species: [Co(H2O)6] 2+ or [CoCl4] 2- or a mixture of both? Based on the color of the initial solution, you can deduce whether K is large or small (the system at equilibrium favors products or reactants). Test tube #1 2. Add 12M HCl solution Prediction: Think about what you actually add to the system! HCl  H+ + ClA solution is added ( a solution is a solute dissolved in water) In effect, you are adding H+ (changes acidity), Cl- (reactant) and water (product) to the system. If more than one factors change, which one has the strongest effect on equilibrium? Test tube #2 1. Add 6M HNO3 solution to the initial solution Prediction: HNO3  H+ + NO3 – A solution is added In effect, you are adding H+ (changes acidity), NO3– (nothing) and water (product) to the system. How is this different than test tube #1, step 2: Addition of HCl? Test tube #3 • Add solid LiCl to saturation (keep adding LiCl until it no longer dissolves). • Prediction: LiCl  Li+ + ClNOT a solution (water is NOT added) Dissociation of LiCl in water is an exothermic reaction (produces heat) Test tube #4 • Add solid NH4Cl to saturation • Prediction: NH4Cl  NH4+ + ClNOT a solution Dissociation of NH4Cl in water is an endothermic reaction (consumes heat) Test tube #5 • Manipulate the temperature without changing concentrations or acidity. • Based on observations, you can conclude whether your system is endothermic or exothermic. • NO NEED TO DO TEST TUBES IN ORDER. Post Lab Assignment – Chemical Equilibrium and Le Chatelier’s Principle CHEM 132L General Instructions The entire report must be typed. You and your lab partner may NOT turn in copies of the same tables/ graphs. Each student must make their own tables/ graphs and answer all questions as an individual effort. Include the following information at the top of the first page of your assignment: Name: Lab Partner(s): Lab Section Number: Experiment Title: Due Date: Data and Calculations 1. Summarize your observations for part A. 2.