• 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

# Factors Affecting the Reaction Rate Between Magnesium and HCL.

Extracts from this document...

Introduction

Factors Affecting the Reaction Rate Between Magnesium and HCL Planning * Hypothesis I predict that as the temperature increases, the speed of the reaction will increase therefore the gas will be produced faster. I believe this because most chemical reactions happen faster when the temperature is higher. At higher temperatures molecules mover around faster, which makes it easier for them to react together. Usually, a rise of 10OC will double the rate of reaction. Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. 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. * Pilot Experiment To decide on the best volume and concentration of hydrochloric acid and best mass of magnesium a number of calculations were done and a pilot experiment conducted. The equation for the reaction is: Magnesium(s) + Hydrochloric Acid(l) Magnesium Chloride(l) + Hydrogen(g) Mg(s) + 2HCL(l) MgCl2(l) + H2(g) We were advised to use 0.1g of magnesium ribbon (found to be 10.9 cm long). The Relative Molecular Mass (RMM) of magnesium is 24, therefore the moles of magnesium to be used was: Moles= 0.1 24 Moles= 0.00416 In the reaction above, 1 mole of magnesium reacts with 2 moles of hydrochloric acid. ...read more.

Middle

A 100cm3 gas syringe should be appropriately accurate for measuring the gas produced since it is accurate to 1cm3 of gas. I will use a three figure balance to measure the mass of magnesium to be used since it is vital that as close to 0.1g of magnesium is used as possible. * Variables I have chosen to repeat the experiment 3 times because it therefore allows me to calculate an average rate of reaction. This will ensure that there are no abnormal results and it will increase accuracy. I have decided to start readings at 20OC and increase by 10OC each time until 60OC is reached, since it will allow me to see the increase in rate of reaction and 5 results should be enough to identify any trends. * Rates of Reaction Increasing the temperature increases the speed of the particles. The faster the particles move, the greater the number of collisions, and therefore the rate of the reaction increases. A 10OC rise in temperature almost doubles the rate of most reactions. Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. 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. ...read more.

Conclusion

Although the initial rate of reaction (which is what I am concerned with in this investigation) seemed to fit a trend, the rate of reaction curves of some temperatures on the graphs crossed. This could have been because some of the magnesium had corroded forming a magnesium oxide layer which would have affected the rate of reaction. Other factor which could have given me unreliable results could have been that the gas syringes were wet causing them to jam and so not giving correct results or that the bung was not placed on the top of the side arm tube fast enough which allowed gas to escape. I conducted all three experiments for each temperature at the same time to save time. An error in my graphs (plotting, drawing curves or calculating gradients) could have also affected the calculated rates of reaction. To improve the experiment I would find a way of attaching and releasing the magnesium inside the side arm tube above the acid (with a bung at the top of the side arm tube) so that the magnesium could be dropped into the acid without any gas being lost. Additional work, which could be carried out, is to repeat the experiment using, a wider range of temperatures. The investigation could also be extended to investigate other factors affecting the rate of reaction such as catalysts, concentration of the acid or particle size of the magnesium. ...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 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. ## Rates of reaction between Magnesium and HCl.

I will therefore use 1M acid and go down by 0.1M, until I reach a 0.1M concentrated hydrochloric acid. As well as this I used a 250ml-measuring cylinder to measure the volume of hydrochloric acid and water needed, but this seemed inaccurate as I need to measure precisely fairly low volume and such a measuring cylinder seemed inadequate.

1. ## Factors Affecting Enzyme Activity

of reaction increases, this is due to the fact that there was more catalase to collide with the hydrogen peroxide in the higher concentrations. One problem with these results is that my control experiment seems to have a rate of reaction however, this is simply due to the initial burst

2. ## Rates of reactions between HCL and magnesium ribbon.

The factors, which may affect how well the experiment works, are how quickly the ribbon is placed in and the stopwatch pressed. Although this is a factor it is not really a major factor that will affect the end results, and as long as the time it all takes is kept constant throughout then it should not matter too much.

1. ## Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric ...

magnesium and hydrochloric acid takes a lot longer than 4 minutes each time, which lower concentrations would. Length of magnesium ribbon Time taken to react 3 cm Over 4 minutes 2 cm Over 4 minutes 1 cm 42 seconds I can see from the above results that the length of

2. ## Find out how different concentrations of HCl affect the rate of the reaction with ...

This is because the loss of mass is so small that it cannot be measured by a 2 decimal place balance. And since we are only provided with 2 decimal place balances I won't be able to follow the rate of the reaction using this method.

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

* Variables I have chosen to repeat the experiment 3 times because it therefore allows me to calculate an average rate of reaction. This will ensure that there are no abnormal results and it will increase accuracy. I have decided to start readings at 20OC and increase by 10OC each

2. ## Investigating Factors Affecting a Chemical Reaction

So collision is unlikely to occur. However, in cases of high temperature, particles take in energy causing them to move faster thus colliding more often hence the rate of reaction is faster As you can see increasing the temperature results in a quicker and faster rate of reaction.

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