• 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

# An Investigation into the Rate of Reaction Between HCL and Mg.

Extracts from this document...

Introduction

An Investigation into the Rate of Reaction Between HCL and Mg Aim The aim of this investigation is to see how concentration of acid effects the rate of reaction between HCL and Mg. The rate of a reaction is how fast the reactants are used up in the reaction. In this investigation we will test different concentrations of acid reacting with magnesium ribbon. Prediction I predict that as the concentration of HCL increases the amount of gas given off by the reaction will increase. Linking Prediction to Theory An increase in concentration is an increase of particles in a given volume. If we increase the concentration 1) The particles are more crowded so they collide more often. 2) The particles themselves do not increase in energy but, there are more particles in the given volume. ...read more.

Middle

= 60ml HCL + 40ml H20 1M = 50ml HCL + 50ml H20 0.8M = 40ml HCL + 60ml H20 0.6M = 30ml HCL + 70ml H20 0.4M = 20ml HCL + 80ml H20 0.2M = 10ml HCL + 90ml H20 I will then measure out 10ml of the HCL solution, then I will add the Mg ribbon, I will try to pay special attention to getting the time exactly so that it is a fair test. I will time for 20 seconds and using the beret I will measure how much gas is given off. I will then repeat the experiment 3 time so that I can get even and average results. Results HCL Concentration Mg Amount (Grams) Time (seconds) Gas Produced (ml) 2M 0.05 20 47 50 53 1.6M 0.05 20 24 24 29 1M 0.05 20 19 19 24 0.5M 0.05 20 8.5 11 13.5 ...read more.

Conclusion

FIG.1 2M HCL 0.5M HCL Evaluation During this investigation there have not been any rouge results and all of our results were as we expected them to be. However our results could not be 100% accurate for several reasons such as our equipment was not 100% accurate, for example our measuring cylinders could have been off by some very small fraction and that could have amounted up. When the reaction takes place bubbles are given off ,which sometimes did stay around the Mg which therefore reduces the surface area of the Mg and so the HCL could not react properly so this could effect the results. We could have controlled the stirring of the solution because if this is not done properly it can lead to incorrect results. Using larger concentrations of acid would give a bigger more accurate conclusion instead of just using 10ml testubes use 1litre testubes, this way graphs would be more spaced out and give a more accurate reading. ...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. ## The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

4 star(s)

The cautions which will be considering are: keeping the level of magnesium and acid to a minimum preventing and hazards, make sure that teachers are informed if there is any hazard present such as spillages or broken glass, make sure no one runs around breaking the boundaries of the teachers

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

However, this does not happen in my experiment and the rates of reaction increase as the temperature increases. However, something which I had predicted does not represent itself in my results. My prediction was, that even though the rate of reaction would increase the final volume of gas collected would be the same for all temperatures.

1. ## Rates of Reaction - HCl + Mg

This is because the acid particles have to collide with the surface of the magnesium. So the larger the surface area, the faster the reaction will be. For the same mass of solid, smaller particles have a larger surface area than larger particles.

2. ## The Rate of Reaction Between HCl and Mg

Hypothetically, there are also several ways to record the results (although we were only given the option of the last way): * Volume of gas evolved- I could use a gas syringe to collect and measure the gas that is evolved from each test of the experiment.

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