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Experiment Plan. Effect of Surface Area on Rate of Reaction

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Introduction

________________ Horizon International School School code: 006048 Session: May 2013 Candidate name: Zwe Kyaw Zwa Candidate number: 006048-004 Subject level: Higher Level Assessment D DCP CE Research Question How does the surface area of calcium carbonate (CaCO3) affect the rate of reaction with dilute hydrochloric acid (HCl)? Hypothesis The rate of reaction of calcium carbonate with a larger surface area will be faster than that of calcium carbonate with a smaller surface area. Background Theory To determine the effect of surface area on the rate of reaction, a known mass of calcium carbonate granules and powder are each placed in a flask, into which standard dilute hydrochloric acid is added. An acid reacts with a carbonate to give a chloride, water and carbon dioxide. Over time, the mass of calcium carbonate decreases while the volume of gas, carbon dioxide, increases. The more gas that is produced in the reaction, the faster the reaction is occurring.This can be measured by means of a graduated gas syringe. ...read more.

Middle

Variables Independent Variable: Size of calcium carbonate Dependent Variable: Volume of carbon dioxide produced Controlled Variables: Temperature Pressure Concentration of dilute hydrochloric acid Mass of calcium carbonate Time interval Control of Variables Variables Identified Type of Variable Treatment Size of calcium carbonate Independent The experiment to investigate the effect of surface area on rate of reaction involves the usage of two sizes of calcium carbonate, i.e., in granules (small surface area) and in fine power form (larger surface area). Volume of carbon dioxide produced Dependent By means of a graduated gas syringe, the volume of carbon dioxide produced is measured and recorded at specific time intervals for reaction involving both calcium carbonate granules and fine powder. Temperature Controlled The experiment will be carried out at constant room temperature (25°C) with a thermometer recording any fluctuation in temperature. Pressure Controlled The experiment will be performed in the laboratory at constant atmospheric pressure(1atm). Concentration of dilute hydrochloric acid Controlled 1M of dilute hydrochloric acid solution will be used throughout the whole experiment. ...read more.

Conclusion

6. At the end of the experiment, a graph of volume of carbon dioxide produced against time is plotted. 7. The same mass (10 g) of calcium carbonate granules are obtained and grounded to fine powder in a mortar using a pestle. 8. The powder is transferred to the flask and the above procedures are repeated, measuring the volume of carbon dioxide produced every 15 seconds interval. 9. Another graph of volume of carbon dioxide produced against time is plotted on the same axes. Table of Results Table 1: Calcium carbonate granules Volume of CO2 (cm3) Time (seconds) Table 2: Calcium carbonate fine powder Volume of CO2 (cm3) Time (seconds) Result Graph Figure: Illustration of rate of reaction by volume of carbon dioxide against time graphs for calcium carbonate granules and calcium carbonate fine powder Discussion The gradient of the curve for calcium carbonate fine powder is expected to be steeper than that for calcium carbonate granules. Therefore, the rate of reaction for the fine powder is likely to be faster than that for the granules. When the reactants are reacted completely, the rate will become constant in both reactions.In this case, the hypothesis is correct. ...read more.

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