Question

Le Chateler's principle

In the chart below: • Indicate the color of each solution as darker or lighter than the control after the addition of the specified substance. • Indicate the direction the equilibrium shifted as "toward products" or "toward reactants" based on the color change. • Based on the direction of the shift, indicate the substance(s) that increased which will either be the two reactants present on the reactant side of the equilibrium equation or the complex present on the product side of the equilibrium equation. Be sure to list the actual substance(s) - do not write reactants or products. Refer to the equilibrium equation: Iodine (aq) + Starch (aq) + Starch - lodine Complex (aq) Yellow-Brown Violet-Black Colorless Tube # Color Substance(s) that Increased Equilibrium Shift 1: control purple 2: + I-KI 3: - Heat 4: + Heat 5: + Amylase

Answer 1

first 4 subparts are answered following HomeworkLib guidelines

Tube color Substance increased Stanch lodine complex starch iodine complen starch-iodine complex 2. +I-KI forward violet black 3. -Heat + beat lodine and yellow-brown yellow-brown 5. iodine to do Acording 3. This is to the right Equilibrium glife 1. control purple Howard prooderet (toward tright) pmduer bonated product violet-black 4. Iloco toward reactant (to the left starch individually tamylase toward deactant due to break down of tarch (orange) percentage of increases with respect starth to de cloetelie's principle, if reactont dis added at equilibrium "seaclin the eam slifts to reduce this stress, it makes more product. an exakumie teretion (well-established). for an exothermie reaction , heat is a proderet. Durering the temperature thrift the rate que 4. Increasing Timp shift the eam to the left (hostant) Anylase completely breakdown startch. By withdrawing sample longer gives violet/ purple color with iodine sol, the io dine soll remains yellow brown A veversible reaction is a a reaction in colide the conversion of reactants to producks comersion of products to renetanto occus Simultaneously; example vapour to form hydrogen iodide. 2. Equilibrium rather chemical equilibrium is the state of where the rate of the forward reaction equals the rate of the reverse reaction. While a rxn is in eau, the concentration of reactants and H2 + 12 → 2HI (famoard) de-chatelier's principle states that if equilibrium a contraint (such' change in Pressure, temperature or concentration of a reactant) /2 HI → Hz + Iz (reverse) is applied to a system for equibrium, the equilibrium will sluft so as to tend to counteract the effect of the constraint. change Effect on equilibrium Increase concentration 70 5. 1. and the the reaction of Hy gars and iodine a reversible reaction constant, constant. products are 3. Rate time shifts to opposite side shifts to same side Decrease cone slights to side with least moles of gas with most 1 4 m n increase pressure decrease pressure increase temperature n in solo endothermic direction exotermic dierease n add a catalyst No change