• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4
5. 5
5

# Investigating The Affect of Concentration on The Rate of Reaction.

Extracts from this document...

Introduction

Name: Laura Thompson Teacher: Mrs. Taylor Investigating The Affect of Concentration on The Rate of Reaction Aim- To find out if changing the concentration of the hydrochloric acid affects the volume of gas released in 5 minutes. Background Information The rate of reaction depends on four things:- 1. Temperature 2. Concentration 3. Catalyst 4. Size of particles/surface area The Collision Theory The collision theory explains the rates of reaction, the rate of reaction depends on how often and how hard the reacting particles collide with each other. The basic theory is that particles have to collide with each other in order to react, but it is not that simple, as it also depends on how hard the particles collide. If the particles do not collide hard enough then they will not react, they will simply just hit each other and 'bounce' off. This means that even if I am not investigating the rate of reaction when the temperature is changed, it will still have a big part to play in my experiment. If the temperature is different in the classroom when I do each concentration of acid it may have a huge impact on my results. To help keep my results as accurate as possible I could take the temperature of the room before I do each experiment. If the temperature in the room is below 20 C the particles will still be moving, but very slowly. This would cause the react to be very slow. At temperatures above 20 C the particles will be moving at a regular speed. ...read more.

Middle

135 Test 2 0.5 16 40 54 88 107 105 108 118 121 123 Test 3 0.5 12 50 71 84 99 105 118.5 129 138 146 Average 0.5 14 50 69 88 102 103.6 112.1 123.3 128.6 134.6 Test 1 1 9 24.5 47.2 70 91 107 123 137 144 155 Test 2 1 10 22 48.5 70 85.6 110 130 136 140 145 Test 3 1 8 18 50 82 90.2 111 135 141 142 149 Average 1 9 21.5 48.6 74 88.9 109.3 129.3 138 142 149.6 Test 1 1.5 20.5 60.7 105 141 174 210 237 260 283 303 Test 2 1.5 20.2 61 101 141 175 211 239 263 286 306 Test 3 1.5 24 67 105 141 174 210 237 260 283 304 Average 1.5 21.6 62.9 103.6 141 174.3 210.3 237.6 261 284 304.3 Test 1 2 93 193 264 346 435 497 519 563 599 637 Test 2 2 90 200 256 360 431 495 520 568 604 626 Test 3 2 99 198 270 350 450 496 529 571 600 619 Average 2 96 197 263.3 352 433 486 522.6 567.3 601 627.3 Any number highlighted are not counted in the average as I believe that the are either to high, to low or do not fit into the pattern. Result that I believe is causing the results for this time to be inaccurate.( see level of confidence) I will not include this result in my new average. I have found out that 2M is the best strength of hydrochloric acid to use when you want a fast reaction, as it released the most gas in 5 minutes compared to 0.5M, 1M and 1.5M. ...read more.

Conclusion

The trend I see from the graph is that the higher the concentration of the hydrochloric acid the steeper the slop of the graph is. I believe that the way in which I carried out my experiment was good as I followed my method exactly. To improve the accuracy of my method I could have said I would use a bulb pipette or a graduate pipette as these are more accurate than a measuring cylinder, I could make sure that the marble chips all have the same surface area because the marble chips with the bigger surface areas could have reacted more than the marble chips with the smaller surface areas. I could have also make sure that the room was the same temperature for each experiment because if the room was hot for one experiment and cold for another then the results would be inaccurate as the molecules would have been moving and reacting at different speeds. The results I have support my conclusion and my prediction, as what I predicted would happen did happen. The order of the concentrations for the most gas released in 5 minutes was also accurate, as it was in the order that I predicted. To extend my investigation I could test if the temperature had any effect on the amount of gas released, I believe this would provide me with the relevant information about what the optimum temperature is for a reaction to take place. I could then test the optimum concentration and the optimum temperature together and see how much gas is released in 5 minutes and compare it to the separate results of the concentration and temperature. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related GCSE Patterns of Behaviour essays

1. ## Close Your Eyes

called again and we realised who it was we broke apart instantly. "Danny!" I gasped, terrified. "Fuck" Dougie replied looking around his wildly. Our clothes were spread over the floor and we were just lying together, naked between the sheets.

2. ## Find out how the rate of hydrolysis of an organic halogen compound depends on ...

For example, a pipette was used because of its high degree of accuracy in quantitative analysis. It has an error of 0.06 cm3 if used correctly (i.e. if it is allowed to drain and retain the last drop). Experiment 2 - - 'Primo' conductivity meter and cell - Calibration solution, HI 70032P - Pipette (with pipette filler)

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to
improve your own work