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# Rate of Reaction Investigations - Decomposition of Hydrogen Peroxide.

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Introduction

Rate of Reaction Investigations Decomposition of Hydrogen Peroxide An aqueous solution of hydrogen peroxide (h202) decomposing very slowly into the water and oxygen. 2H2O2 (aq) 2H2O(l) +O2 (g) Task Hydrogen peroxide decomposes very slowly into water and oxygen. The Manganese (iv) oxide is a catalyst for the reaction. Therefore it speeds up the reaction speeds up the reaction (but is not used up itself). The factors (variables) that affect the speed of this reaction are the concentration of the solution h202. A reaction goes faster when the concentration is increased. The effect of temperature of on a reaction is that, when the reaction is increased so does the speed. The effect of the surface area on the rate of a reaction is that, when the surface area of a solid reaction or catalyst is increase, so does the speed .The Manganese (iv) oxide (catalyst). Catalyst is substance that speed up the rate of reaction. Catalyst are not used up or changed. The variable that I plan to control in this experiment are the temperature, catalyst, surface area and time. The variable that I plan to change is the concentration. Prediction I predicted that the stronger the concentration the faster the rate of reaction. ...read more.

Middle

Average (s) 1st 2nd 3rd (cm3) 0 0 0 0 0 30 23* 27 29 28 1:00 40* 51 50 51 1:30 52* 67 67 67 2:00 62* 79 81 80 2:30 69* 90 90 90 3:00 75* 97 100 99 3:30 80* 100 100 100 4:00 84* 100 100 100 4:30 87* 100 100 100 5:00 91* 100 100 100 Concentration 0.5M Time Volume oxygen produced (cm3) Average (s) 1st 2nd 3rd (cm3) 0 0 0 0 0 30 30* 37 37 37 1:00 55* 67 71 69 1:30 73* 91 92 91 2:00 87* 100 100 100 2:30 90* 100 100 100 3:00 99* 100 100 100 3:30 100 100 100 100 4:00 100 100 100 100 4:30 100 100 100 100 5:00 100 100 100 100 Concentration 0.6M Time Volume oxygen produced (cm3) Average (s) 1st 2nd 3rd (cm3) 0 0 0 0 0 30 47 40* 46 47 1:00 75 70* 75 75 1:30 98 90* 96 97 2:00 100 100 100 100 2:30 100 100 100 100 3:00 100 100 100 100 3:30 100 100 100 100 4:00 100 100 100 100 4:30 100 100 100 100 5:00 100 100 100 100 * = Odd results Calculating the gradient 0.2M 11cm3/30s = 0.37cm3/s 0.3M 20cm3/30s = 0.67cm/s 0.4M ...read more.

Conclusion

Because there are more collisions, the reaction rate is greater. Catalyst - the catalyst seem to lower the activation energy for the reaction. Many more collisions are 'successful', and the reaction is faster. Exactly how the catalyst achieves this remains a mystery for many reactions. When I look back at my prediction I could see my result and what I predicted were some concentration did increase with time, eventually at a point where it got used up. Looking at my result I can see that the rate changes with time. The graph is steepest at the start of the experiment, showing the rate of the reaction is greater than. As the reaction continues, the rate decreases until, eventually. The reaction stops. This is happening because in the solution of higher concentration and in gases of higher pressure, particles are closer together. They have a greater chance of colliding because they are more collisions, that rate of reactions greater. Conclusion In the experiment I have investigated how different levels of concentration affect the rate of reaction. After I finish my experiments, I found out a pattern of result on my graph and data. Which was as the concentration level increases, the rate of reaction also increases. In solution of higher concentration, the particles are crowded together. They have a greater chance of colliding. Because there are more collisions, the reaction rate is greater. ...read more.

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