Hypothesis: I hypothesis that the enzyme concentration will affect the rate of reaction but only up until a certain point because there is a limited supply of substrate. Enzymes are protein molecule that acts as biological catalyst by increasing the rate of reactions without changing the overall process. They are long chain amino acids bound together by peptide bonds. Enzymes are seen in all living cells and controlling the metabolic processes in which they converted nutrients into energy and new
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Effect of Temperature on Solubility of a Salt Ahmed Mohammed 17-nov-2013 Abstract In this experiment‚ you will study the effect of changing temperature on the amount of solutet will dissolve in a given amount of water. In this experiment‚ you will completely dissolve different quantities of potassium nitrate‚ KNO3‚ in the same volume of water at a high temperature. As each solution cools‚ you will monitor temperature using a computer-interfaced Temperature Probe and observe
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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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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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Determining Order from Rates of Reactions AP Chemistry Purpose The focus of this experiment is to recognize that when aqueous solutions of potassium iodate ion (KIO3-) and bisulfite ion (HSO3-) are mixed‚ a series of reactions will occur‚ and the final reaction is signaled by the appearance of a dark blue color. My partners and I investigate how the concentration of the reactants affects the rate of reaction. The purpose of this lab is to find
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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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purpose of laboratory assignment 3 was to measure the rate at which a chemical reaction takes place. For the purpose of this lab we measured the rate a balanced oxidation/reduction reaction between iodine‚ hydrogen‚ and bromate ion occurs. The above reaction occurs slowly so we used a coupled iodine clock reaction to measure the rate of the oxidation/reduction reaction because it occurs much faster but is still dependent upon the other reaction. To accomplish this‚ two mixtures were prepared in separate
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Aim: To determine the rate law of chemical reactions Introduction: The aqueous solution of potassium peroxydisulphate can oxidize potassium iodide as follow: Equation: K S 0 (aq) + 2KI (aq)->2K S0 (aq)+I (aq) 2 2 8 2 4 2 KI(aq) +I (aq) -> KI (aq) 2 3 _________________________________________________ K S 0 (aq) +3KI(aq) -> 2K S0 (aq)+ KI (aq) 2 2 8 2 4 2 The rate law of this reaction can be represented as follow: Rate=k[S208 2-]^a [I-]^b When the concentration of peroxydisulphate ions
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Chemical reactions proceeding until all the reactants are used is a common misconception. Chemical reactions actually behave differently. The general reaction equation is a A + b B → c C +d D in this equation A and B are the reactants forming the products C and D. However‚ unlike the common thought that the reaction ends when it runs out of A and B it actually does not. In most reactions C and D start to react to form A and B at a certain point as you can see in the equation c C + d D → a A + b
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will increase the speed of reaction as the greater the surface of the solid reactants‚ the more particles are required to expose and ‘cover’ the capacity of the solid. Increased surface area results in an increased chance of collisions between reactant particles. Since the collisions become more frequent and abundant‚ the rate of reaction increases. Aim The aim of the experiment is to see if a greater surface area of a dissolvable tablet creates a faster or slower reaction Independent Variable
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