• 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 Factors Affecting the Rate of a Chemical Reaction

20 (23) - room temperature 231 0.004 30 (32) 125 0.008 40 (42) 55 0.018 50 (50) 37 0.027 60 (61) 22 0.045 Here is a graph of the preliminary results Here I have found results that can now aid me in making my prediction. The Experiment APPARATUS 0.03 moles/dm3 of THIO 2 moles/dm3 of HCL acid Mixing beaker (heat resistant)

2. ## Investigate the factors affecting the rate of a reaction.

I am going to make each different concentration of hydrochloric acid myself by using 1 molar hydrochloric acid and distilled water to dilute when needed. Using the measuring cylinder, I will add however much water is needed to the hydrochloric acid to make it 0.2 molar, 0.4 molar, 0.6 molar, 0.8 molar or which ever strength is needed.

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

I will then repeat the experiment for the rest of the concentrations. I will then repeat the whole experiment again and take the average of both results for each concentration. Other factors are what kind of water to use for dilution, I could either use water from the tap which

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

PREDICTION AND HYPOTHESIS I predict (using information earlier in this section) that as you increase the temperature the rate of reaction will increase. This is because the heat energy, which is supplied to the atoms, is converted into kinetic energy and therefore the atoms move and collide with each other causing reactions.

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

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.

2. ## Factors Affecting Enzyme Activity

to get exactly the right amount of it due to its consistency I have decided to further investigate the liver suspension as a source of catalase. Although in the experiment the liver was too efficient catalysing the reaction too quickly I believe this is due to the fact that the

1. ## Investigation Into the Factors Affecting Rate of Reaction

I chose to measure the rate of reaction on calcium carbonate with hydrochloric acid. I found that when the concentration is increased, the rate of reaction increases. The equations for this experiment were: CaCo3 (s) + 2HCl (aq) CaCl2 (aq)

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

The ionic equation for the reaction is: Mg (s) + 2H (aq) 2Cl�(aq) ----------> Mg�(aq) 2Cl�(aq) + H2(g) The chlorine is a spectator ion. So the equation is: Mg (s) + 2H (aq) ----------> Mg�(aq) + H2(g). Mass of 10cm of Mg = 0.08g. Mass of 1cm of Mg = 8 � 10��g.

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