How Fast Is Your Reaction

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How fast is your reaction?

Part 1 – How temperature affect the rate of reaction
Chemical equation
Magnesium + hydrochloric acid → magnesium chloride + hydrogen Mg + 2HCL → MgCl2 + H2

Graph

Conclusion and questions
1. What factors/variables did you keep the same in this experiment?

* We kept the same volume of hydrochloric acid (10 cm3) and the magnesium ribbon (5cm) because that way we could get a fair test experiment. We also repeated the experiment twice.

2. What does increasing the temperature do to the rate of reaction?

* In my results I found out that the rate of reaction increases as we increase the temperature. For instance at 30°C the rate of reaction is 0.006 seconds and at 60°C the rate of reaction is 0.017 seconds. This means that the lower the temperature is the faster is the reaction.

3. What conclusion can you make about the rate of this chemical reaction?

* The rate of reaction increases when the temperature increases. So doubling the temperature almost doubles the rate of reaction. This is the reason that the rate of reaction increases from 30°C, 0.009 to 60°, 0.017.

4. How does increasing the temperature affect the hydrochloric acid molecules that react with the magnesium atoms in this chemical reaction? Use particle diagrams in your answer.

* When we increase the temperature the particles start to collide and bump to each other. They have more energy and that affects the rate of reaction.

5. Using the chemical equation, write down the following : a) The reactants
b) The products
c) The state of matter of all the reactants and products
d) If the chemical reaction is reversible or irreversible. a) And b) Magnesium + hydrochloric acid → magnesium chloride + hydrogen.

Reactants products c) Mg – solid HCL – liquid MgCl – solid H – gas d) ireversible

6. Using the chemical equation for the reaction, write down the names and numbers of each atom taking part. Make a table like the one shown below you: Name of Atom| Chemical Symbol| Number used in the chemical reaction| Magnesium| Mg| 1|

Chlorine| Cl| 2 | Hydrogen| H| 2|

Part 2 – How concentration effect the rate of reaction
Chemical equation
Sodium thisulphate + hydrochloric acid → sulphur + sulphur dioxide + sodium chloride + water. Graph

Conclusions and questions.
1. What factors/variables did you keep the same in this experiment? * We kept the volume of hydrochloric acid (10 cm3) the same. The concentration of sodium thiosulphate affects the rate of reaction. 2. What does increasing the concentration of sodium thiosulphate do the rate of reaction? * Increasing the concentration of sodium thiosulphate increased the rate of reaction.

3. What conclusion can you make about the rate of reaction?
* The rate of reaction increases as the concentration of sodium thiosulphate increases. The more we put of sodium thiosulphate the rate of reaction increases, the less water we put the rate of reaction increases. The greater the concentration of sodium thiosulphate the faster the rate of reaction. The rate of reaction was the fastest at 40 (g/dm3) of sodium thiosulphate. However we did get one weird result at 24mml of sodium thiosulphate. It was higher than we expected it would be. To improve the experiment we would repeat it more times and calculate the average result. 4. How does the concentration of sodium thiosulphate affect the rate of reaction? Use particle diagrams in your answer. * Increasing the concentration of sodium thiosulphate we increase the rate of reaction. When we increase the concentration there are more...
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