• 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
7. 7
7
8. 8
8
9. 9
9

# INVESTIGATION INTO THE REACTION RATE BETWEEN MAGNESIUM AND HYDROCHLORIC ACID

Extracts from this document...

Introduction

INVESTIGATION INTO THE REACTION RATE BETWEEN MAGNESIUM AND HYDROCHLORIC ACID Joseph Colledge Contents Page(s) Introduction 1 Method 2 Results Tables 3 Graphs 4-13 Description of Results 14 Discussion 15-16 References 17 Introduction An underlying principle on which all of the sciences of kinetics are built is the law of mass action which states that the rate of a chemical reaction (which is basically how fast the speed is of a reaction, not how much product is made) is proportional to the active masses of the reacting substances. Due to the complications in measuring active mass it is much easier to dilute the solutions as then the active mass can be replaced by the concentrations. This principle means that the rate of a chemical reaction is, therefore, proportional to the concentrations of the various reactants. The concentration of a solution can be seen as how strong the solution is, for example if we consider the reaction between Magnesium and Hydrochloric acid: Mg + 2HCL --> MgCl2 + H2 The stronger an acid the more acid particles and less water particles than a weaker acid, so increasing the concentration of a solution works on this same principle in that it increases the chances of collisions occurring between the two reactants. ...read more.

Middle

As hypothesised originally, the table shows a direct correlation between the amounts of Mg placed into the 2.0M HCL and the amount of H2 produced. In the columns for 2cm and 3cm of Mg it can be seen that there is a gradual increase in the amount of Hydrogen produced. Whereas in the columns for 4cm, 5cm and 6cm there is a large increase with the amount of Hydrogen produced even at 5 seconds is double the amount produced with the 2cm and 3cm of Mg. Table 2 shows the levels of Hydrogen produced when the amount of Mg remains a constant (at 4cm) whilst the concentration of the HCL is diluted as described in the method. The results as shown in table 2 corroborate with the hypothesis also, in that as the level of molarity in the hydrochloric acid decreases so does the amount of hydrogen which is produced. This is shown in table 2 as at 2M the reaction is producing large amount of hydrogen whereas when studying the amounts which are produced from the 1.6, 1.2, 0.8 and 0.4 dilutions you can see massive reductions in the amount of hydrogen produced so much so that when the dilution is at 0.4 there is barely any hydrogen produced at all. ...read more.

Conclusion

One of the most obvious places where error could occur is in the dilutions of the hydrochloric acid in the second part of the experiment as due to the very nature of dilutions it makes it possible for human errors to creep into the results. To improve on the results I would recommend completing each section of the experiment at least twice and comparing the results of each, or if that wasn't possible to pool the results of all the groups and take an average of them all. Also it may be prudent to use distilled water for the dilutions, as using water directly from the tap may change the pH to a greater level than is required for the experiment. Also I believe that the positioning of where the experiment was being carried out would have a direct result on the results found as the intensity of the light is a lot more obviously a lot more intense at the window whereas it is more subdued at the other side of the laboratory. In conclusion, the results of the experiment clearly concurred with the hypothesis in the introduction in that basically the concentration of the reactants in the experiment has a direct influence on the products given off. ...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)

7 6.33 0.07 120 8 7 8 7.67 0.06 150 10 11 10 10.33 0.07 180 13 14 13 13.33 0.07 Safety Safety/Risk Assessment: For this investigation I will take specific cautions when investigating how different concentrations effect rate of reaction, this will be done before we start with our experimentation in order to fulfil our investigation.

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 reactions between HCL and magnesium ribbon.

First of all, the particles of the reacting substances must collide with each other and, secondly, they need a certain amount of energy to break down the bonds of the particles and form new ones. This energy is called the activation energy or Ea.

2. ## Rate of reaction of hydrochloric acid and mangesium ribbon.

Scientific Knowledge "When a chemical reaction occurs, the particles which combine need to meet up with each other (collide) so that they can swap or share electrons. If you want to speed up a reaction, you need to get these particles to hit each other more frequently." (www.revise.it) ? ?

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

R Method for different acids. * Make the different concentrations of H2SO4 and CH3COOH using the method show under "method for different concentrations". * Then add 10cm� of 2M H2SO4 into a test tube. * Add 1cm of magnesium to this test tubes.

2. ## Study the reaction kinetics and find out evidence about the mechanism between the reaction ...

Units of Rate Constant Zero - d [A] d t = k [A] = [A]0 - k t [A] vs t - k mole dm-1 sec-1 First - d [A] d t = k [A] [A] = [A]0 e- k t ln [A] vs t - k sec-1 Second -

1. ## The aim of this investigation is to find out the effect of concentration of ...

A change in concentration is a change in the number of particles in a given volume. If we increase the volume a)the particles are more crowded so they collide more often. b)even though the average amount of energy possessed by a particle does not change, there are more particles

2. ## Find out the effect of concentration of acid, in thereaction between dilute hydrochloric caid ...

During a chemical reaction the particles have to collide with enough energy to first break the bonds and then to form the new bonds and the rearranged electrons, so it�s safe to say that some of the particles don't have enough energy to react when they collide.

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