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An Investigation to show the factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid

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Introduction

An Investigation to show the factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid Introduction: The collision theory says that successful collisions can only take place when there is enough activation energy, which is caused by particles colliding together head on with enough energy to break the existing bonds to form new ones. When a successful collision occurs a reaction will take place. Aim: In this experiment I will be investigating whether temperature and concentration affect the rate of reaction between magnesium strips and hydrochloric acid. Hypothesis: I predict that as the concentration 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 concentration is higher. At higher concentrations molecules are closer together, which makes it easier for them to collide. Because there are more collisions, the reaction rate is greater. Chemical reactions take place by chance. ...read more.

Middle

6. All these concentrations were recorded twice for accuracy. It was important that only the concentration was changed because this was what was being investigated. Temperature: 1.I measured 100cm3 of hydrochloric acid and added it to a beaker. 2.Using a Bunsen burner and a thermometer I warmed up the acid to the required temperature. 3.Then I measured 5 cm of magnesium ribbon and cleaned it using emery cloth by rubbing it up and down the strip. After the magnesium had been cleaned I placed it in the warm acid. 4. The stopwatch was started as soon as the magnesium ribbon was added to the acid. When it had all dissolved the timer was stopped and the time recorded. 5.I then repeated the experiment for acid of temperatures 23C, 30C, 35C, 40C and 45C using a Bunsen burner to heat the acid. 6. All these concentrations were recorded twice for accuracy. In this experiment, it was important that only the temperature of the acid was changed because this was what was being investigated in this experiment. ...read more.

Conclusion

Also in the 2.0M solution compared with the 1.0M solution there are much more HCl particles in the same volume so the are going to collide with each other more often Therefore I predict that the rate of reaction will increase with the concentration of the HCl solutions. 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. Since there are more collisions the chemical reaction takes place faster. Results: Concentration (mols) Temp (C) Time 1(s) Time 2 (s) Average (s) Reaction rate ...read more.

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