• 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

# How does the temperature affect the rate of reaction for magnesium?

Extracts from this document...

Introduction

How does the temperature affect the rate of reaction for magnesium? Aim - My aim is to find out how temperature affects the rate of reaction with magnesium. Prediction - I predict that the higher the temperature of the acid, the quicker the reaction with magnesium will take place; the lower the temperature the slower it will take place. Science - I believe this because, when two chemicals react, their molecules have to collide with each other with sufficient energy for the reaction to take place. This is collision theory. The two molecules will only react if they have enough energy. By heating the mixture, you will raise the energy levels of the molecules involved in the reaction. Increasing temperature means the molecules move faster. This is kinetic theory. So by heating the particles up the magnesium particles will collide harder with the hydrochloric acid, causing it to dissolve faster, whereas if it was at room temperature it might take longer to dissolve, as the particles do not have as much energy. ...read more.

Middle

Fair Test - To keep it a fair test, the variables need to be kept the same to prevent getting the wrong results. The temperature of the acid needs to be accurate to get the correct rates of the reacting magnesium. The Hydrochloric acid cannot be used again after the reaction otherwise the acid will be less strong to act on the magnesium. We will try and use the same amount of magnesium for each reaction; however they are not the same length. The temperature range will be ten degrees in between each other as this is not Method - First of all I am going to sort the apparatus out as necessary. Apparatus: * Bunsen Burner * Tripod * Conical flask * Stop clock * Gauze * Thermometer * Hydrochloric acid * Magnesium strips Now I am going to test the rate of reactivity of the magnesium with hydrochloric acid at room temperature. I added 20ml of hydrochloric acid into the conical flask and had the stopwatch ready to start timing, the magnesium was then added. ...read more.

Conclusion

Evaluation - In this experiment we encountered many problems; problems that might have caused the two anonymous results in the second test. This may have been because the magnesium pieces were not exactly the same size or some of the hydrochloric acid wasn't washed out properly, also water might have been in the conical flask. This will have weakened the concentration of the acid therefore slowing the reaction with magnesium, and giving us our odd results. We could have avoided this by washing the conical flash out thoroughly with water, and then drying it with a paper towel. Also the reaction might have taken longer at a higher temperature because we left the Bunsen burner under the conical flask for too long, therefore the temperature being too high, caused the particles to react too much - dissolves magnesium too fast. This could have been avoided by taking the Bunsen burner from under the conical flask before it reached the temperature, as the gauze is still hot and heated the conical flask. Rachel Boyes ...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. ## How dose temperature affect the rate of reaction between magnesium and hydrochloric acid.

3 star(s)

On page 79 in the relative section this is what I found: "When the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more collisions." The second relative quote was on the same page: "The rate of a reaction simply depends on how

2. ## Rates of reactivity.

* Both substances within the reaction were liquids so to control the surface area it will be very difficult. * No catalysts would be used. * I will use the same standard of time judged when the 'X' has disappeared.

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