Factors affecting the rate of reaction between a metal and an acid The rate of a reaction can be measured by the rate at which a reactant is used up‚ or the rate at which a product is formed. The temperature‚ concentration‚ pressure of reacting gases‚ surface area of reacting solids‚ and the use of catalysts‚ are all factors which affect the rate of a reaction. Individual properties of substances also affect reaction rates. The scope of these properties is broad and there are few generalizations
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percentage errors. OBJECTIVE The objective of this experiment is to determine the order with respect to permanganate ion and to oxalic acid concentration for the reaction of potassium permanganate and oxalic acid solutions. Other goals include‚ writing a rate equation and determining the effect of increased temperature on the rate of this reaction. MATERIALS AND EQUIPMENT The materials required for this experiment include the following: • 2-50ml Burets • 60 mL of 0.755M H2C2O4 • 60 mL
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hypothesis proposed that if a small amount of salt was added to the reaction‚ then it cause the rate of the reaction to speed up‚ but if too much salt was added‚ then it will instead decrease the rate of the reaction. The data revealed that no additional amount of salt was the reaction that had the highest rate. As shown previously in the data table‚ the first trial’s average reaction rate of 4.5 mL/min was higher than the other two reaction rates where salt was added for trial 2 and trial3‚ 2.125 mL/min and
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− ( − 6 ) = _______ − 2 − 10 = _______ − 8 − ( − 8 ) = _______ − 8 − 8 = ________ m. − 16 − 11 = _______ Last night the temperature in New York City went down to 4°F. In Antarctica‚ the temperature went down to − 20°F. What is the difference between the two temperatures? answer: _____________ In Antarctica‚ the temperature air temperature is − 5°F . The temperature of the nearby water is 33°F. How much colder is the air than the water? answer: _____________ Super Teacher Worksheets − www.superteacherworksheets
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Given the evidence‚ it can be determined that a reaction will occur when reactants have a kinetic energy greater than the activation energy‚ this is a theory of collision theory. For example‚ in the first experiment‚ the test tube filled with 10 mL of 3% hydrogen peroxide and had scoop of manganese dioxide‚ had a greater reaction than the other test tube. Which simply contained 10 mL of 3% hydrogen peroxide. The factor that affected the reaction rate was that the manganese was seen as a catalyst.
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graph‚ you can see that there is a relation between the rate of reaction and the surface area. The larger the surface are‚ the faster the rate of reaction seems to be. However‚ although the grain with the largest surface area (the smallest grain) reached the highest point within the shortest amount of time‚ its end result was still lower then the medium sized grain. The explanation for this result is relatively easy. The rate of a chemical reaction can be increased by increasing the size of the surface
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(Tinnesand‚ n.d.). A strong acid ionises completely while a weak acid only ionises partially. Furthermore‚ the strength of the acid will also have an effect on the rate of the reaction. A strong acid will have a faster reaction then
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the substances used in respiration (sugar or oxygen) and the waste products created. The breakdown of glucose also releases carbon atoms‚ which become available for biosynthetic reactions‚ enabling the yeast to grow and reproduce by budding or fission. The rest of the carbon ends up in the by-products of these reactions‚ such as carbon dioxide‚ ethanol‚ and other more minor
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factors affecting the rate of a chemical reaction. Introduction: In my coursework I will be mainly concentrating on the reaction between dilute hydrochloric acid with marble chips (calcium carbonate). Calcium carbonate (marble chips) + hydrochloric acid ==> calcium chloride + water + carbon dioxide CaCO3(s) + 2HCl (aq) ==> CaCl2 (aq) + H2O (l) + CO2 (g) Aim: The aim of the experiment is to investigate how the concentration of hydrochloric acid affects the rate of reaction with marble chips‚
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An investigation to show how the rate of reaction between hydrochloric acid and sodium thiosulphate is affected by the concentration of the acid Simple Procedure Place a conical flask on a piece of paper with a cross on it. Add hydrochloric acid and sodium thiosulphate‚ and record the amount of time taken for the cross to disappear through the solution from the top of the flask. Record this time and repeat this for different concentrations of hydrochloric acid. Fair Test The variables in
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