• 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 rates of reaction

Extracts from this document...

Introduction

Coursework - Investigating rates of reaction Aim: To see what effects changing the concentration of hydrochloric acid will have in a reaction between magnesium and hydrochloric acid. Prediction: The higher the concentration of acid, the faster the rate or reaction will be. Background Info: The phrase "rate of reaction" means "how fast is the reaction" or "the speed of the reaction." Rates of reaction can vary from very slow reactions such as rusting to very fast reactions such as magnesium dissolving in hydrochloric acid (the investigation I am doing). There are things that can speed up reactions; they are called catalysts, which can be a transition metal or an enzyme which reduces time to save money. There is a rate equation to show the rate of reaction, it is: The overall order of reaction is given by (a + b), a or b usually have values such as 0, 1 or 2. If the order of reaction is 0, then as the concentration increases, the rate will not be affected; If the order of reaction is 1, then as the concentration is doubled then so is the rate; If the order of reaction is 2, then as the concentration is doubled then the rate is multiplied by 4. ...read more.

Middle

1 Minute 1 Minute 30 Seconds 2 Minutes 0.25 0 25 8 7 10 14 18 0.25 5 20 8 5 8 11 14 0.25 10 15 8 4 5 6 8 0.5 15 10 8 5 7 10 13 0.5 20 5 8 1 1 1 1 N/A 25 0 8 0 0 0 0 Results: Concentration of Acid = 1 Mole Conc. Length Time R.T Water cm Acid cm Mg 30 60 90 120 150 180 210 240 270 300 20 0 25 6 cm 47 73 83 83 83 83 83 83 83 83 20 5 20 6 cm 30 55 68 75 81 81 81 81 81 81 20 10 15 6 cm 11 24 34 45 54 61 66 66 66 66 20 15 10 6 cm 5 10 15 23 28 32 37 42 46 50 20 20 5 6 cm 2 4 6 8 10 12 14 17 19 21 20 0 25 6 cm 49 79 82 82 82 82 82 82 82 82 20 5 20 6 cm 38 64 83 93 99 99 99 99 99 99 24 10 15 6 cm 21 37 50 61 70 77 82 88 88 88 24 15 10 6 cm 11 ...read more.

Conclusion

It therefore shows a more similar pattern to the results in the first run than the second run. There were only 2 runs taken, because the results from the first run were so successful and went so smoothly I thought a second run would only further show what I already knew, just make it more certain and reliable. This was so, except I didn't expect the change in room temperature to affect the results as much as it did, it doesn't make the results any less certain; it just shows how much the temperature can affect the rate of reaction. I recorded the results every 30 seconds for five minutes because I believed that five minutes was enough time for the reaction work fully, which in the higher acid concentration cases it was; I took results at 30 second intervals because this was enough time for a sufficient amount of gas to be produced, making it a fairer test. If I could have repeated this experiment again, I would have taken 3 runs with different temperatures for each, to show how much the temperature can affect the rate of reaction. ?? ?? ?? ?? ...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. Investigating making Epsom salts by varying the rates of reaction.

reaction was happening too quickly so in the space of 30 seconds 40cm of water would have been lost, and we were finding that before 210 seconds all the water was finished ,we did not believe it at first so we started up another experiment along side one and it

2. Investigating Rates of Reactions

HCl particles, therefore there would be less number of HCl particles colliding with Mg particles so there would be less successful collisions, causing a reduction in the rate of reaction. And this causes a reduction in the amount of hydrogen gas being produced because if we dilute the acid with

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