This lab focused on three factors affecting reaction rates‚ temperature‚ surface area‚ and concentration. Our first experiment (table 1) looked mainly into the effects of temperature on the reaction rate. To see how different temperatures would change the reaction rates we had three flasks all containing varying temperatures of water(H20). One with cold water (4°C)‚ one room temperature (21°C)‚ and one with hot water (44°C). In each flask‚ we dropped one tablet of Alka-Seltzer‚ all within 0.008 grams
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Reaction Rate Coursework Aim To see how the concentration of a reactant affects the rate of reaction‚ in this case sodium thiosulphate and acid. Scientific Background For a reaction to occur‚ the particles of the reactants must be colliding with each other with enough energy‚ the amount of energy needed for the reaction is called activation energy. Activation energy is altered by temperature‚ concentration‚ surface area of and the pressure on the reactants. Stirring the reactants also increases
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which more clearly displays the relationship‚ view Figure 2. The rate at which the reaction occurred for the 100% concentration is 1.45 mg/dL per minute. For the 50%‚ the rate was 3.05 mg/dL per minute‚ and for the 25%‚ the rate was 2.76 mg/dL per minute. As seen‚ the rate fluctuated from the lowest rate at 100% and the greatest rate occurring at 50%. As mentioned earlier‚ the Collision Theory states the rate of a chemical reaction is proportional to the number of collisions that occur. One way to
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Changing the Rate of Reaction PART 1: PARTICLE SIZE Question: How does changing the particle size of marble (CaCO3) affect the rate of reaction when it is added to hydrochloric acid (HCl)? Hypothesis: If I change the particle size of marble to test how to change the rate of a chemical reaction‚ than the chemical reaction with the smallest marble particles will produce CO2 the quickest because the larger the surface area‚ the more place the hydrochloric acid will have to collide with the marble
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Factors that Affect the Rate of Reaction of Peroxidase Purpose: To determine the effect of various factors on the rate of reaction between an enzyme and its substrate‚ and also to determine the optimal ranges under which the enzyme activity is maximized. Also to determine whether saline and alcohol are inhibitors or activators Hypothesis: PH factor prediction: I predict that as the pH increases so the activity of the enzyme will increase until it reaches optimum pH range (pH 7) because the
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The rate of a chemical reaction is the measure of change in concentration of the reactants of the change in concentration of the products per time. The rate of a chemical reaction is influenced by the concentration of the reactants‚ temperature‚ and the presence or absence of a catalyst. Through finding the time and concentrations of the reactants‚ it is possible to find the rate of reaction and k. To perform this experiment‚ you need two erlenmeyer flasks‚a timer‚ a LabQuest with a temperature
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Abstract The following experiment details the effect of different concentrations of catalase on the production of oxygen and water through the breakdown of Hydrogen Peroxide. In this experiment paper disc where coated in varying concentrations of catalase‚ 0‚ 25‚ 50 75 and 100%. The time taken for the disc to float between two markers on the side of a glass was then recorded. This experiment demonstrates that the higher the concentration of enzyme used the greater the production of oxygen on the
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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: The rate at which a reaction occurs‚ or takes place‚ is affected by various factors‚ such as the temperature at which the experiment is conducted in‚ the pressure which is given‚ the surface area which is exposed‚ use of catalysts‚ and the concentration. In this investigation‚ I would be investigating the affect of surface area‚ or particle size‚ in the rate at which a reaction occurs. Background Information: The more finely divided the solid is‚ the faster the reaction happens. A powdered
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Study of the first element – Hydrogen. Answer the following questions:- 1. Give a reason why hydrogen can be placed in group 1[IA] and group 17[vIIA] of the periodic table. 2. What similarities does it show with group 1[IA] and group 17[VIIA]. With special reference to valency electrons and ion formaton and examples. 3. How does hydrogen occur in the free and combined state? 4. Which metals react with cold‚steam and boiling water to form their respected oxides and hydroxides ? Give examples and
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