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Investigating The Rates Of reaction Between Magnesium Ribbon And Hydrochloric Acid

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Introduction

Investigating The Rates Of reaction Between Magnesium Ribbon And Hydrochloric Acid Aim I am trying to show that the rate of reaction between hydrochloric acid (HCl) and magnesium (Mg) can be varied. Variables My Variables are: 1) Light 2) Pressure 3) Temperature 4) Concentration 5) Catalyst 6) Surface Area The variables can be changed in the following ways: 1) Light works in basically the same way as temperature, as light heats the space around where the experiment is taking place. 2) The greater the pressure the closer the particles are forced together. This means there are more collisions, which in turn increases the rate of reaction. Pressure would only affect the experiment if one or more of the involved reactants are of gaseous state. 3) The higher the temperature, the faster the rate of the reaction, this is due to the fact that the higher the temperature is the more energy each particle has, this makes the particles vibrate more causing more collisions with greater activation energy. ...read more.

Middle

It is a shiny grey metal. It is of solid state. Hydrochloric acid (HCl) is an acid of about 35% hydrogen chloride, it is very corrosive and safety precautions should be taken. Goggles should be worn at all times while using this substance. It is of gaseous state. Prediction I predict that as the concentration level increases the rate of reaction will increase also. The greater the concentration, the more particles. The more particles the more chance there will be of more collisions. The more collisions the faster the rate of reaction. Apparatus I will need the following apparatus for the experiment: 15 Test Tubes A Test Tube Rack 2 Pipettes A Timer 2 molar Hydrochloric acid 15 pieces of magnesium ribbon each 0.5cm long Water Diagram Test Tube solutions Concentration In Moles 1 = 2 2 = 1.5 3 = 1.2 4 = 1 5 = 0.5 Method Measure and cut 15 pieces of magnesium ribbon into 0.5cm long pieces. ...read more.

Conclusion

1 4:20:09 0.5 2 18:37:11 9:28:40 0.5 3 5:28:40 Analysis My prediction was correct according to my results in the above table. The rate of reaction increased as the concentration increased. This is because there are more particles and allowing more collisions, which in turn speeds up the rate of reaction. Conclusion I have found a pattern in my results that is also followed by my averages I have formed. The pattern is that the rate of reaction is proportional to the concentration. The greater the concentration, the more collisions, which causes a faster reaction rate. Evaluation To further prove that the theory 'the greater the concentration the faster the rate of reaction' I would need to make a better and stronger conclusion. I would also need to improve my investigation and be more accurate in taking the readings. I could take more readings for a more precise average and could use different variables. I could have measured the mass of the magnesium ribbon for a more accurate set of results. ...read more.

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