Kenishia Pascal 10x3. Investigating How Different Concentration Effects The Rate Of Reaction. Strategy A Possible Factors * Source of catalase * Concentration * Surface Area of enzyme * Concentration of enzyme * pH * Temperature Chosen Factor We chose to investigate the concentration of enzyme as we had previously investigated the optimum temperature for catalase in the preliminary investigation. Concentration of enzyme is also fairly easy to investigate‚ as
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Purpose: To find out the densities and to find out the name of the unknown metals. (Based on the extensive and intensive properties) Check up the words mass‚ volume‚ density‚ extensive properties‚ and intensive properties. Where do the units for mass and volume) come from and what do they mean? What is the density of distilled water? What is Archimedes principle? Does temperature affect the density of a solid? Liquid? Gas? Materials: Safety glasses‚ 10‚ 25 or 50 mL graduated cylinders
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Chemical reactions are a part of everyday lives. Whether it is the burning of propane at a kitchen stove‚ or washing detergent reacting with dirt stains‚ chemical reactions are useful tools that have widespread applications. With so many reactions assisting our everyday activities‚ it is important that ways to optimise reaction rates are investigated. “Reaction rate‚ the speed at which a chemical reaction proceeds… may be defined in terms of the amounts of the reactants consumed or products formed
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Kinetics 6.1 Rates of reaction 6.2 Collision theory 6 16.1 Rate Expression (AHL) 16.2 Reaction mechanism (AHL) 16.3 Activation energy (AHL) 6.1 Rates of reaction 6.1.1 Define the term rate of reaction. 6.1.2 Describe suitable experimental procedures for measuring rates of reactions. 6.1.3 Analyse data from rate experiments. © IBO 2007 Figure 601 An explosion is a quick reaction D ifferent chemical reactions occur at different rates (i.e. speeds). Some
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alcohols with the presence of a catalyst. A carboxylic acid contains the -COOH group‚ and in an ester the hydrogen in this group is replaced by a hydrocarbon group of some kind. Sulfuric acid (H2SO4)is used as a catalyst for this reaction in order to accelerate the rate at which the product is formed. The general formula of an ester is RCOOR’ in which R is the alkyl group that comes from the carboxylic acid while R’ is the alkyl group that comes from the alcohol and COO is the functional group of
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There are three reactions in the iodine clock reaction. The first reaction is IO3-(aq) + 3 HSO3-3 SO4-(aq) + I-(aq)+ 3 H+(aq)‚ where the iodate ions become iodide ions1. The second reaction is 6 H+(aq) +IO3-(aq) + 5 I-(aq) 3 I2(aq) + 3 H2O(l) where the iodate ions become molecular iodine2. The third reaction involves molecular iodine becoming a dark blue starch;I2(aq) + starch blue-black complex3. These three reactions react in a sequence. In any reaction the concentration is exponentially related
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Experiment to investigate the effect of concentration of electrolyte on the current of voltaic cell Aim The aim is to identify the relationship between the concentration of H2SO4 solution and the current of Cu-Zn voltaic cell. Hypothesis My hypothesis is that the greater the concentration of sulfuric acid the bigger the current of the voltaic cell. In a voltaic cell‚ chemical energy is concerted to electrical though the oxidation and reduction happen on the electrodes. Current will not flow
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how the change in solvent polarity affects the rate and to determine the kinetics of a solvolysis reaction. In this experiment‚ we used 1-chloro-1-phenylethane in acetone in one reaction with 50% ethanol-50% water and in another reaction with 40% ethanol-60% water. To monitor he rate of reaction‚ we would need the concentration of the alkyl chloride at the beginning of the reaction and at a time t‚ but since we did not determine the concentrations‚ we monitored the rate of formation of HCl since
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RATE OF REACTIONS. The reaction rate (rate of reaction) or speed of reaction for a reactant or product in a particular reaction is intuitively defined as how fast or slow a reaction takes place. For example‚ the oxidative rusting of iron under the atmosphere is a slow reaction that can take many years‚ but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second (right). Chemical kinetics is the part of physical chemistry that studies reaction rates. The concepts
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Chemistry 521 Exam I‚ Spring Quarter 7:30 - 9:00 PM‚ 25 April 2000 NAME 1. [10 points] What are the concentrations of HSO− ‚ SO2− ‚ and H+ in a 0.20 M KHSO4 solution? (Hint: 4 4 H2 SO4 is a strong acid; Ka = 1.3 × 10−2 for HSO− .) 4 2. [15 points] Calculate the pH of 1.00 L of the buffer 1.00 M CH3 COONa/1.00 M CH3 COOH (pKa = 4.74) before and after the addition of (a) 0.080 moles NaOH and (b) 0.12 moles HCl. (Assume there is no change in volume). 3. [10 points] The following reaction
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