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Investigate the rate of reaction between HCl and Na2S 2O3

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Planning Investigate the rate of reaction between HCl and Na2S2O3 Jackie Randall 10A For this piece of coursework we are investigating the rates of reaction and he effect different changes have on them. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction. We are studying the affect of changing concentration of Na2S2O3 Solution and dilute HCl. I believe these variables will affect the rate of reaction: * Surface area * Pressure * Temperature * Catalyst * Concentration Concentration If the concentration of a solution is increased there are more reactant particles per unit volume. This increased the probability of reactant particles colliding with each other. Pressure If the pressure is increased the particles in the gas are pushed closer. This increases the concentration and that will change the rate of reaction. Surface Area If a solid is powdered then there is a greater surface area available for a reaction, compared to the same mass of unpowdered solid. ...read more.


I also predict that as the concentration of the sodium thiosulphate increases the rate of reaction will increase. When the temperature is increased the particles will have more energy and this would enable them to move faster. This will make them collide more often and with more energy. Particles with more energy are more likely to overcome the activation energy barrier to reaction; this would make them react successfully. If solutions of reacting particles are made more concentrated there are more particles in the area. Method Experiment 1 - Changing the concentration 5 cm3 of HCl (at concentration 1 mol./dm3) and 15 cm3 of sodium thiosulphate (at varying concentrations - 10 to 35 g/dm3) are poured out into two measuring cylinders and then poured into a conical flask, which is placed on top of a board marked with letter X. The stopwatch will now be started. When the mixture has turned sufficiently cloudy so that the letter X can no longer be seen the stopwatch will be stopped and the time will be recorded. ...read more.


As the solution gets more concentrated the ions are closer together therefore they will collide more often and more successful collisions are likely, therefore as the concentration decreases fewer successful collisions take place and the rate of reaction slows. Apparatus List * Water Bath * Hazcards * Plastic Pipette * Beaker (250cm3) * Wash bottle * Distilled water * Measuring cylinder (100cm3 and 10cm3) * Flask (250cm3) * HCl (1 Molar) * Stopwatch * Na2S2O3 What I Will Do With My Results... With the results I will use them for creating the following items: * Plot some graphs (Perfect curve, line of best fit) On the axes, I will write: The rate (y axes) and Average time (x axes). * I will also plot the following graph: average times (y axes) and concentration of a) Na2S2O3 b) HCl Strange Results... Potential Variables...Anomalies These are results that are completely out of the blue and therefore most likely to be wrong! I will keep a close eye out for these in my experiments and if I do spot any the experiment will be repeated. ...read more.

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