• 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
6. 6
6

# What factors affect the rate of reaction of Magnesium and Hydrochloric acid.

Extracts from this document...

Introduction

Rate of Reaction Aim: What factors affect the rate of reaction of Magnesium and Hydrochloric acid. Prediction: I predict the rate of reaction of Magnesium and Hydrochloric acid will increase as the temperature increases. I also predict that the rate of reaction of Magnesium and Hydrochloric acid will increase when the surface area of the Magnesium is increased and the concentration of the Hydrochloric acid is increased. Hypothesis: The Collision Theory describes the way temperature, concentration and the surface area of the solid reactant affects the rate of reaction, by affecting the collision between particles. Particles react when they collide with enough velocity and sufficient energy. I predict the rate of reaction of Magnesium and Hydrochloric acid will increase when the temperature increase. This is because changes in temperature change the kinetic energy of the particles and hence the numbers of successful collisions with enough energy to break existing bonds and make product parties. The minimum energy needed for a successful collision is called the activation energy. For a reaction to take place reagent molecules must collide with each other. When they do so, they must seize enough energy to cause or initiate a reaction. The level of energy needed to start a reaction is called its energy barrier. ...read more.

Middle

General formula: Magnesium (s) + Hydrochloric acid (l) Magnesium Chloride (l) + Hydrogen (g) Mg (s) + 2HCl (l) MgCl2 (l) + H2 (g) Method 1 (Temperature): * Add 25 ml of (2 molar) Hydrochloric acid in to a conical flask * Heat it by putting it in a water bath * When the acid reaches 60�C, add a strip of (5 centimetre long) Magnesium to the acid * Use a stop watch to time how long it will take before the Magnesium strip dissolves I used the same method for 40�C and 27�C (room temperature). Method 2 (Concentration of acid): * Add 25ml of (0.5 molar) Hydrochloric acid in to a conical flask * Add a strip of (5 centimetre long) Magnesium to the acid * Use a stop watch to time how long it will it take before the magnesium strip dissolves I used the same method of 1 molar and 2 molar of Hydrochloric acid. Method 3 (Surface area): * Add 25ml of (1 molar) Hydrochloric acid in to a conical flask * Add a strip of (1.25 centimetre long * 4) of Magnesium to the acid * Using a stop watch time how long it will take before the Magnesium strip dissolves I used the same method for 2.50 centimetre long * 2 and 5 centimetre long magnesium strips. ...read more.

Conclusion

But in my hypothesis I said that the when the temperature is doubled it would half the time then the temperature before but it did not happen. This shows that when the temperature is doubled, the time don't take half the time then the temperature before. My 'Concentration of acid' result shows us that when concentration of the acid is increased the rate of reaction increases rapidly. It took an average time of 15:16 sec for the Magnesium to dissolve when the concentration was 0.5 molar, whereas it only took 3:14 sec when using 1 molar and 0:25 sec when using 2 molar. Again in my Hypothesis I said that it would take half the time when you double the concentration then the concentration before but it took much more time than I thought it would. My results don't show a pattern but it shows that there is a dramatic change when the concentration of the acid is increased. My 'Surface area' result shows that there is a slight difference when there is an increase with the surface area. Although I think that this is inconclusive because my 2.50 centimetre long * 2 strip takes less time than the 1.25 centimetre long * 4 strip. ...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)

To investigate how temperature rices in different amounts of acid with different lengths of magnesium carried out a little experiment and collected data that helped to solve this problem and decide on what the amounts should be in the finally practical.

2. ## How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

I accurately measure the time that had elapsed to the nearest second with the stop clock. Did I take enough readings? Not enough concentrations were used for a good graph. I should have used concentration 3M acid ought to have been done but it was not known then that it was necessary and required.

1. ## Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

If you look at the diagram of the apparatus you will see that the pipe leading to the gas syringe from the chronicle flask is ascending. We also know that hot air rises. Therefore, the hotter the hydrochloric acid, the hotter the air in the flask and the hotter the gas the leaves the reaction will be.

2. ## How does changing the concentration of hydrochloric acid affect its rate of reaction with ...

In the less concentrated solution, there are fewer acid particles, which means that there is a smaller chance of them colliding with the magnesium atom. The particles will eventually react, but at a slower rate. In the highly concentrated solution, there are more acid particles for the reaction to take place much quickly.

1. ## An Investigation into the factors affecting the rate of reaction between magnesium and hydrochloric ...

As the temperature is increased the particles move faster since they have more energy. This means that they are colliding more often and more of the collisions have enough velocity to cause a reaction. Since there are more collisions the chemical reaction takes place faster.

2. ## Investigating the affect of concentration on the rate of reaction between magnesium and hydrochloric ...

area * Temperature * Presence of a catalyst * Concentration/pressure if gaseous The surface area of the solid reactants can be changed which has a big effect on the rate of reaction. For example magnesium powder will react faster with hydrochloric acid than magnesium ribbon.

1. ## Does concentration affect the rate of reaction between magnesium strips and hydrochloric acid?

The faster collisions will lead to a faster rate of reaction, therefore the higher the concentration, the faster the rate of reaction will be. This is because compared to a 0.5 molar acid, a 5 hydrochloric acid has more particles to react with and therefore more heat will be given

2. ## 'Investigating factors that affect the rate of chemical reactions.'

collecting cylinder is necessary to collect the gas and allow its volume to be measured. In addition a stopwatch and a balance is needed to make the measurement of time and weight accurate and so to control the variables. Conical flask with side arm Stopper Glass tube Beaker of water

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