Finding the rate law was the overall goal of the laboratory. When finding the wavelength of the Azo Orange II dye‚ the highest wave was the point used‚ 483nm. The plotted points of the different concentrations absorbance’s made sense to have a steady upward slope because the dye was diluted in steady increments from full to ¾ and so on. Beer’s law was used next to calculate the absorbance of they time over time as bleach was added. One the absorbance value was calculated‚ the concentrations were
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on the rate of reaction. By using self investigative and experimental skills‚ the experiment was done in order to determine how the rate of reaction will be altered‚ whether it will increase‚ decrease or remain constant when the different concentration of enzymes added. INTRODUCTION: Enzymes are produced naturally in plant‚ animal‚ and microbial cell. There are thousands of different enzyme can be found in any cell. Enzymes can be describe as molecules that are greatly increase the rate of chemical
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concentration on the reaction between Catalase and hydrogen peroxide. Introduction Enzymes are proteins that act as catalysts (a substance that increases or decreases the rate of a reaction) 2. Enzymes bind to a molecule called a substrate‚ converting it into a product. Nearly all of the chemical reactions that occur in a biological cell need enzymes to make them occur. Enzymes like all catalysts lower the activation energy needed for a reaction to take place3. They dramatically speed up the rate at which
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Investigate the effect of concentration on the rate of a reaction Research question: To what extent does the concentration of hydrochloric acid affect the rate of the following reaction: 2 HCl(aq) + CaCO3(s) → CaCl2(aq) + H2O(l) + CO2(g) Data Collection and Processing: Table1: Different volumes of Co2 gas produced by Different concentrations of HCL acid. Volume of CO2gas formed from 5 different concentrations of HCL acid ±0.5ml 5 different concentrations of HCL acid (Mol) ±0.5ml Time (sec) ±0
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Affect Rates Of Reaction Aim: How does the mass of calcium carbonate affect its rate of reaction with hydrochloric acid? Hypothesis: I hypothesize that when the mass of the calcium carbonate increases‚ the rate of reaction of the calcium carbonate and hydrochloric will also increase. The collision theory states that the more successful collisions there are within the reaction‚ the faster the rate of reaction. When the mass increases‚ so does the number of particles in the reaction‚ thus
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Alka-Seltzer Reaction Rates Lab What are the different factors the effect the reaction rate of Alka-Seltzer? Matthew Arkfeld Leah Gilligan Jessie Abbott Period 4 June 2nd‚ 2008 Background Research: o The objective of the experiment was to determine if different factors affect the reaction rate of Alka-Seltzer. Alka-Seltzer provides fast relief to acid indigestion‚ upset stomach‚ heartburn‚ headaches‚ body aches and pains. It is an antacid and pain relief medicine used by millions
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Lab Report: How Temperature affects Reaction Rate Aim: The Aim is to investigate how temperature can affect Reaction Rate. The experiment will be performed by heating equally sized and weighted lime stones with equal amounts and concentration of Hydrochloric acid at different temperatures. The temperatures will be 35˚C and 40˚C. We will measure the reaction rates by observing gas release of the reaction between lime stones and Hydrochloric acid. The amount of gas release at different
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and neutralise stomach acid. Planning Aim To determine how the surface area of the tablets affects the rate of the reaction. To determine which form of tablets gives the biggest surface area resulting in the fastest reaction rate. Investigation question: What is the relationship between the total surface area of the tablets and the rate of the reaction? Hypothesis: The rate of reaction will be the fastest when the tablets crushed into powder as there is a bigger total surface area resulting
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Name: |Date:| Exp 1: Observations of Chemical Changes|Lab Section: | Data Tables: Part 1: |Chemicals|Well No.|Observations of the Reaction| A.|NaHCO3 + HCl| H12|White and bubbled slightly and settled down to smaller smaller bubbles| B.|HCl + BTB| H11|Golden yellow; looked darker under the black paper| C.|NH3 + BTB|H10 |Dark blue| D.|HCl + blue dye| H9|Greenish color| E.|Blue dye + NaOCl| H8|Blue and lighter than NH3+BTB solution color| | with the 1 drop of HCl| H8|Turned blue green
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Acquisition of a Second Order Reaction Abstract Introduction The rates at which reactions occur depend on the composition and the temperature of the reaction mixture. Usually the rate of reaction is found to be proportional to the concentrations of the reactants raised to a power.1 There are many reactions that have a rate law in the form of: (1) v = k[A]a[B]b According to reference1 the power to which the concentration of a species (product or reactant) is raised in a rate law of this nature
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