How the Concentration of Hydrochloric Acid Changes the Rate of the Reaction with Magnesium

How the Concentration of Hydrochloric Acid Changes the Rate of the Reaction with Magnesium
Aim The investigation that I will be doing is to investigate the rate of reaction between Magnesium and Hydrochloric acid. Factors which will effect this experiment will be ? The concentration of the acid because as you increase the concentration of acid you will also increase the change of an collision so there for speeding up the reaction ? Temperature. As you increase the temperature you will also increase the rate of the reaction because the particles move around with more energy so a greater chance of an reaction. ? Surface area. This will also effect the rate of collision because there is more surface area able to react with the acid so increasing the chance of an collision Prediction I predict that when I increase the concentration of the acid I will notice an increase in the rate of the reaction. This is because there is a greater chance of HCl particles reacting with an Mg atoms. This is because If the concentration of any reactant in a solution is increased, the rate of reaction is increased. Increasing the concentration, increases the probability of a collision between reactant particles because there are more of them in the same volume. Apparatus ? A gas syringe
Hydrochloric acid ? Magnesium ? Stop watch ? Beaker ? A flask ? Rubber bung ? Measuring cylinder Diagram -?? Method 1. a measuring cylinder with 50 ml of hydrochloric acid and pour it in to a flask 2. Add three 2cm strips of magnesium to the flask. 3. attach the rubber bung with the gas syringe to the flask 4. start the stopwatch 5. record the volume of gas every 10 seconds 6. repeat this experiment altering the concentration of the Hydrochloric acid by adding the following amounts of water 50ml HCl 0ml of water 40ml HCl 10ml of water 30ml HCl 20ml of water 20ml HCl 30ml of water 10ml HCl 40ml of water Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Time seconds 10 20 30 40 50 60 70 80 90 1st exp 15 27 38 48 60 68 74 77 80 2nd exp 15 25 35 45 60 68 74 77 80 average 15 26 37 47 60 68 74 78 80 Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Time seconds 10 20 30 40 50 60 70 80 90 1st exp 6 12 18 25 32 38 44 49 54 2nd exp 8 14 20 27 34 39 45 50 55 average 7 13 19 26 33 39 45 50 55 Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Time seconds 10 20 30 40 50 60 70 80 90 1st exp 3 6 9 12 15 17 21 24 26 2nd exp 3 6 10 13 16 19 22 25 27 average 3 6 10 13 16 18 22 25 27 Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Time seconds 10 20 30 40 50 60 70 80 90 1st exp 1 2 3 5 6 8 10 11 13 2nd exp 1 2 4 5 7 9 11 13 14 average 1 2 4 5 7 9 11 12 14 Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Vol (ml) Time seconds 10 20 30 40 50 60 70 80 90 1st exp 0 0 1 2 3 3 4 4 5 2nd exp 0 0 1 1 2 3 3 4 4 average 0 0 1 2 3 3 4 4 5 Analysis My graph shows just what I thought the higher the concentration the acid was the faster the reaction. The graph shows that the reaction to slow down after about 60 seconds with the 50ml of 1m HCl. This is because the number of reactants is being used up so the rate of reaction starts to slow down. This could also be said for the other experiments if I had enough time. One thing I have noticed is that the jump from 10ml water +40 ml of HCl and 50mlof HCl is almost double at each average time and this happens all the way through the results. So over all my prediction was correct as the concentration of the HCl increases so does the rate at which H gas is produced this is because there is a greater chance of HCl particles reacting with Mg atoms. Evaluation -???- Looking at my graph there are no anomalous results and all of the results seem to be within 1 or 2 cm of each other and there seem to be no cause for concern. The volumes also finished up at roughly the same after 90 second. The improvements that I could do if I was to do the experiment again would be: 1. You need two people to place the Mg in the HCl and start the stopwatch. 2. When you place the rubber bung in to the flask the air is displaced and pushes the gas syringe out. 3. The Mg stuck to the side of the flask so not reacting as well with the HCl. 4. Dry the flask out after washing because the water could dilute the acid slightly . Future investigations that I could of used is a bigger variable to get a wider variable to get a wider range of results such as from 0.05m to 2m going up 0.05m each time. This is so that there would be a wider range of results so that I could see a trend much more clearly. So an over all look back at my experiment: ? The reliability was good because non of the results are out or strange. I repeated every one twice and got similar results ? The accuracy none of the point lie very far from the line of best fit so the results were accurate ? I think that there is enough evidence because I feel the results are reliable enough and show me what I need to know and thought.

How the Concentration of Hydrochloric Acid Changes the Rate of the Reaction with Magnesium 8.2 of 10 on the basis of 2000 Review.