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Investigating the Effects of Surface Area on the Rate of Reaction

Extracts from this essay...

Introduction

Investigating the Effects of Surface Area on the Rate of Reaction ________________ ________________ Aim: To study the effects of changing the surface area on the rate of a chemical reaction Hypothesis: This hypothesis is based on the Collision Theory, where in order to react, the two particles involved must: 1. Collide with each other 2. The collision must be energetic enough to overcome the activation energy of the reaction 3. The collision must bring the reactive parts of the molecule into contact the correct way â they must collide with appropriate geometry (the reactive parts) Considering that the surface area of a particle is a factor that mainly affects the collision rate of particles, it would be safe to assume that as the surface area increases, the reaction rate increases. The graph should turn out to be something like this: 1. the reaction is the fastest at the start 2. The reaction is slowing down here 3. No more product is formed Amount of product Time Variables: Variable Factor What is manipulated Dependent Time The time it takes for the reaction to complete depends on the surface area of the compounds being used, because it determines the rate in which the reaction will occur.

Middle

This divided by 2 equals 0.05 s Data Presentation Graphs Processed Data Magnesium Ribbon Experiment 29.00±0.05+41.00±0.05+34.00±0.052=34.70 ±0.05 s 36.00±0.05+55.00±0.05+43.00±0.052=44.70 ±0.05 s 41.00±0.05+65.00±0.05+50.00±0.052=52.00 ±0.05 s 45.00±0.05+76.00±0.05+55.00±0.052=58.70±0.005 s 47.00±0.05+80.00±0.05+63.00±0.052=63.30 ±0.05 s 52.00±0.05+87.00±0.05+72.00+0.052=70.30 ±0.05 s 35.00±0.05+95.00±0.05+76.00±0.052=79.30 ±0.05 s 70.00±0.05+98.00±0.05+84.00 ±0.052=84.00 ±0.05 s 77.00±0.05+101.00±0.05+88.00±0.052=88.70 ±0.05 s 81.00±0.05+108.00±0.05+91.00±0.052=93.30 ±0.05 s Magnesium Ribbon Experiment â the average of the results Volume in cm3 (±2.5) Time in seconds (±0.05) 5 34.70 10 44.70 15 52.00 20 58.70 25 63.30 30 70.30 35 79.30 40 84.00 45 88.70 50 93.30 Calcium Carbonate â The Marble Chips Experiment 29.00±0.05+27.00±0.052=28.00 ±0.05 s 43.00±0.05+45.00±0.052=44.00 ±0.05 s 52.00±0.05+61.00±0.052=56.50±0.05 s 64.00±0.05+79.00±0.052=71.5 ±0.05 s 76.00±0.05+96.00±0.052=86.00±0.05 s 91.00±0.05+110.00±0.052=100.50±0.05 s 99.00±0.05+128.00±0.052=113.50±0.05 s 110.00±0.05+143.00±0.052=126.50±0.05 s 124.00±0.05+157.00±0.052=140.50±0.05 s 128.00±0.05+171.00±0.052=149.50 ±0.05 s 136.00±0.05+187.00±0.052=161.50±0.05 s 148.00±0.05+199.00±0.052=173.50±0.05 s 156.00±0.05+213.00±0.052=184.50±0.05 s 165.00±0.05+231.00±0.052=198.00±0.05 s 177.00±0.05+243.00±0.052=210.00±0.05 s 194.00±0.05+258.00±0.052=226.00±0.05 s 208.00±0.05+273.00±0.052=240.50±0.05 s 221.00±0.05+290.00±0.052=255.50±0.05 s 231.00±0.05+304.00±0.052=267.50±0.05 s 243.00±0.05+319.00±0.052=281.00±0.05 s Calcium Carbonate â The Marble Chips Experiment Volume in cm3 (±2.5) Time in seconds (±0.05) 5 28.00 10 44.00 15 56.50 20 71.50 25 86.00 30 100.50 35 113.50 40 126.50 45 140.50 50 149.50 55 161.50 60 173.50 65 184.50 70 198.00 75 210.00 80 226.00 85 240.50 90 255.50 95 267.50 100 281.00 Sodium Carbonate â The Powder Experiment 3.00±0.05+2.00±0.052=2.50±0.05 s 6.00±0.05+3.00±0.052=4.50±0.05 s 13.00±0.05+5.00±0.052 =9.00±0.05 s Sodium Carbonate (Powder Experiment)

Conclusion

For example, if I used magnesium, to study the effects of surface area on the rate of reaction, I would only you magnesium ribbon and magnesium powder. Studying different elements with different reactivityâs would dismiss any data already collected because an elementâs position on the reactivity series may also determine the rate of reaction. Use the same element. 1. Amount of People involved in the experiment 1. If I had to do the experiment again, with the same apparatus, I think I would like to have 3 people participating in the collection of data. 1 person would be watching the syringe rise and call out to record whenever it rose, the 2nd person would time it, and the 3rd person would record it. This time, the data may be even more accurate, because no one is taking their eye off the experiment, like I was doing during my experiment just to record data. I feel that altering these aspects of the experiment would increase the level of accuracy, as to get more substantial data to calculate the order of reaction. Unfortunately with the data I have so far, I am unable to derive the concentrations of the substances I had utilized in my experiment. However, as the objective was to investigate whether or not different surface areas affected the rate of the reaction, I think that I have produced enough data to support my theory. By Jade Waqaliva

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