Name: Yaissa Fernandez 4.05: Chemical Reactions Data and Observations: Complete a data table that includes a prediction of reaction type‚ observations‚ and identification of reaction type for each reaction in the lab. (10 points) Reactants Prediction of Reaction type Observations Reaction Type Iron (III) and Copper (II) Sulfate Solution Single replacement Solids stay concentrated at the bottom Single replacement Lead (II) Nitrate and Potassium Iodide Solutions Double replacement Yellow powder
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flask with an iodine crystal with a bromobenzene solution with a stir bar. Once the stirring began‚ the solution turned brown and over time began to lighten up. The color change to brown indicated that the reaction began and this is why an iodine crystal was placed in the solution. The reaction started to boil due to its own reflux so heat didn’t need to be applied. Next the anhydrous ether solution was added very slowly in a dropwise manner with a needle through the septum cap on the condenser. This
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Virtual Lab: Enzyme Controlled Reactions Worksheet 1. Which of the following does NOT apply to an enzyme: Inorganic 2. When an enzyme catalyzes a reaction: Substrate(s) bind in the active site 3. Which of the following would interfere most with the ability of an enzyme to catalyze a reaction? Reduced concentration of substrate available 4. Feedback mechanisms regulate the rate of enzyme activity‚ effectively “turning off” an enzyme
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Introduction Nivaldo J. Tro describes kinetics as the study of how changes that occur in chemical reactions take place over time‚ and because of its vast utilization in a multitude of industries‚ it may be one of the most significant and fascinating aspects in the entire chemical world. One application of the study of kinetics can be applied to the determination of the rate of a chemical reaction involving a certain selection of chemicals (FD&C Blue #1 and sodium hypochlorite). The purpose of the
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is being released or absorbed in a chemical reaction. My lab partner and I had to determine the heat exchanged when solid magnesium hydroxide is mixed with solid citric acid‚ using a coffee cup calorimeter. Given that citric acid is soluble in water is the property that makes this reaction possible. The first law of thermodynamics and Hess’s law are also present within this experiment. Knowing the difference between endothermic and exothermic reactions is also relevant. If the temperature goes down
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Investigating the effects of changing concentration: iodine clock reaction. Abstract This is an experiment to show the Iodine Clock Reaction. To create a chemical reaction to see how long it takes for solution to change to a dark blue Color. When changing the concentration of the iodide (K1) and adding distill water to make it up to 5cm³ each time. This is to see if the reaction takes less with less concentration or faster with more concentration added to the peroxodisulphatee. So with the solution
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The Rate of a Reaction The area of chemistry that deals with the rate or speed of chemical reactions is known a chemical kinetics. The word “kinetic” is derived from the Greek name kinitikos that means movement or motion. In the present context‚ the kinetic means the reaction rate or rate of a reaction that is defined as the change in concentration of a reactant or a product with time (M/s). Chemical reaction can be represented by the following general equation. Reactants Products It is very important
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CHEM 206- ORGANIC CHEMISTRY EXP 10-UNIMOLECULAR ELIMINATION REACTIONS Cansın Etli Lab Instructor: Emel Yılgör Experiment date:06.12.2010 Report Date: 20.12.2010 ABSTRACT In this experiment‚ the purpose was to investigate E1 elimination mechanism with the reaction of cyclohexanol to cyclohexene. The reaction was acid catalyzed dehydration of alcohol and with catalyst sulfuric acid cyclohexene was obtained from cyclohexanol. And the product
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Analysis of a Chemical Reaction Purpose: To observe a chemical reaction and to use qualitative and quantitative evidence to identify this reaction from among four possibilities. Hypothesis: I think the result is going to produce water. I think this is going to happen because there is hydrogen and oxygen inNaHCO3. Materials: -Test tube clamp - 150 mm test tubes (2) - burner - retort stand - clay triangle - iron ring - crucible Procedure: Part A: 1. Add 0.5 g of NaHCO3
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- low value for current passing Strong bases : group 1 hydroxides (ie NaOH etc)‚ or lower group 2 hydroxides Ba(OH)2. - good conductors Weak bases : NH3‚ CH3CH2NH2. - poor conductors Reaction rates Similarly‚ the rate of reaction will reveal the strength of an acid. The rate of a chemical reaction is usually proportional to the concentration of the reactants. As it is the hydrogen ions that
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