Chemical equilibrium

Introduction The point of this experiment is to calculate an equilibrium constant for a chemical reaction by watching “Le Chatelier’s Principle” works in this experiment with iron (II) thiocynate. Le Chatelier's Principle is defined as, “A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change” (Purdue Web). Two things can happen within these shifts to relieve stress: The first one is the

Chemistry 12 Santa Monica College Determination of Kc for a Complex Ion Formation Objectives • • Find the value of the equilibrium constant for formation of FeSCN2+ by using the visible light absorption of the complex ion. Confirm the stoichiometry of the reaction. Background In the study of chemical reactions, chemistry students first study reactions that go to completion. Inherent in these familiar problems—such as calculation of theoretical yield, limiting reactant, and percent yield—is

Objectives 1. To recognize the macroscopic properties of five chemical systems at equilibrium 2. To observe shifts in equilibrium concentrations as stresses are applied to the systems. 3. To observe a shift in equilibrium concentrations associated with changes in temperature. 4. To explain the observations obtained by applying Le Chatelier’s principle. Materials Refer to page 209 of Heath Chemistry Laboratory Experiments. Procedure Refer to pages 209 – 211 of Heath Chemistry

Determining the Ksp of Calcium Hydroxide by Titration of Saturated Ca(OH)2(aq) with HCl(aq) Abstract: Titration is a technique that has been used in this experiment to identify the Ksp value of calcium hydroxide in order to determine the extent to which the compound is soluble in water. A known volume of 50 mL of hydrochloric acid, a concentration of 0.05 M hydrochloric acid, a volume of 50 mL calcium hydroxide base, an unknown concentration

ability of PDMS to release absorbed chemicals into water. In general, experiments have proven that PDMS can be used to calculate the equilibrium concentrations of many different compounds dissolved in water once the concentrations of these analytes absorbed in the pellets are determined. Since PDMS is not affected by the nature of the matrices or by exposure to hydrophilic chemicals, it can be used for

solubility product constant (Kₛₚ) of calcium hydroxide (Ca(OH)₂) by using the concentrations of calcium and hydroxide found during titration. The solubility product constant, or Kₛₚ, represents the level at which a substance dissolves in a solution at equilibrium. A higher Kₛₚ value means the more soluble a substance is in a solution. The solubility product constant, similar to solubility, is temperature dependent. When writing the expression for Kₛₚ solids and liquids do not appear since their concentrations

Title: “The Effect of Substrate Concentration, Enzyme Concentration, pH and Temperature on Enzyme Activity” Abstract: In the following experiments we will measure precise amounts of potato extract as well as Phenylthiourea, combined with or without deionized water and in some instances change the temperature and observe and record the reaction. We will also investigate the different levels of prepared pH on varying samples of the potato extract and the Phenylthiourea and record the results.

Enzymes are central to every biochemical process. Due to their high specificity they are capable of catalyzing hundreds of reactions that signifies their vast practical importance. This experiment was conducted to investigate the enzymatic activity of the enzyme aldolase by using different urea concentrations. Stronger solutions of denaturant in this case urea were used to increase the polypeptide subunit unfolding and the dissociation of the tetramer. Aldolase is an enzyme that consists of four

Plant materials and stress treatment Twelve barley varieties available in Bangladesh Agricultural Research Institute (BARI) were selected for the determination of their antioxidant activity during saline stress. Varieties are: Bari barley -1, Bari barley -2, Bari barley -3, Bari barley -4, Bari barley -5, Bari barley -6, Bari barley 7, BHL-10, BHL-12, BHL-15, BHL-19, and BHL-26. Seedlings were grown in field condition and were imposed to a certain level of salinity. Data were taken on different parameters

Graph 6a (Substrate) – Represents a xy scatterplot with linear regression, which show the change in product concentration over the change in time at different substrate The data in the graph also gives the value of V0 at corresponding substrate concentration. Graph 6b (Substrate) – Represents a xy scatterplot depicting velocity of enzyme-catalyzed at multiple substrate concentrations. To find the concentration of the different absorbance in this experiment, a modified version of the Beer’s Law