2 0 Moles Concentration example essay topic

Rate of Reaction Aim: To find out how different concentrations change the rate of reaction Theory: In this experiment the collision theory is in use. It means that when the concentrates solutions of hydrochloric acid is use, more particles are found in the same space, which means they are more likely to collide with each other. the more the concentrated the solution, the more of the collisions with the particles, which increases the rate of reaction. Prediction: As the concentration of the solution increases the rate of reaction increases with it Hypothesis: The reason I think that my prediction is right, is because I know that more concentrated the solution is, the quicker the reaction will happen. List of equipment: In this experiment I will use boiling tube, measuring cylinder, timer, hydrochloric acid (0.5, 1.0, 1.5, 2.0, 2.5, 3.0 Moles), magnesium, test tube rack, clamp stand, a ruler and i will have to wear goggles to protect my eyes. Preliminary test: The thing I will change is the concentration of acid What I will measure is the time that it takes gas to reach 5 cm 3 Things I will keep the same is the amount of solution and the length of the magnesium Method: Firstly I will set my experiment as shown on the next page will make sure everything is straight I will get all of my 6 different solutions, every time I use a solution I will measure 10 cm 3 of it and every time I will use two pieces of magnesium of length 10 mm I will measure time it takes the gas to get to 5 cm 3 and hopefully it will work, then I will measure time until it gets to 10 cm 3 Table of results for preliminary: concentration Time it takes to get to 5 cm 3 of gas 0.5 M 0.83's 1.0 M 0.18's 1.5 M 0.12's 2.0 M 0.01's 2.5 M 0.02's 3.0 M 0.01 sIn my preliminary I found it hard to take the right time when I was waiting for the gas to reach 5 cm 3 because the reaction happened really fast so I think that may be a reason why I got an anomaly so now I will measure the time it takes to get to 10 cm 3 of gas. I also will repeat the experiment twice just to make sure results are reliable. concentration Time it takes to get to 10 cm 3 of gas 0.5 M 0.219's 1.0 M 0.42's 1.5 M 0.15's 2.0 M 0.07's 2.5 M 0.10's 3.0 M 0.06's concentration Time it takes to get to 10 cm 3 of gas 0.5 M 0.410's 1.0 M 0.511.

5's 0.315's 1.0 M 0.42's 0.51's 0.46. 5's 0.47's 1.5 M 0.15's 0.16's 0.15. 5's 0.16's 2.0 M 0.07's 0.06's 0.06. 5's 0.07's 2.5 M 0.10's 0.05's 0.07. 5's 0.08's 3.0 M 0.06's 0.04's 0.05's 0.05 sI have found the average's so I can draw a graph for it, I have also rounded up the averages so it is easier to draw a graph for it.

Now I'm going to work out the rate of reaction. To get that I need to divide 1 by the time that I got for my experiment. i have already rounded up my averages but I will round them up even more concentration average Average rounded up 0.5 M 0.315's 0.32's 1.0 M 0.47's 0.5's 1.5 M 0.16's 0.2's 2.0 M 0.07's 0.1's 2.5 M 0.08's 0.1's 3.0 M 0.05's 0.1 rate = 1/time 0.5 Moles'a 1/0.32 = 3.13 1.0 Moles'a 1/0.5 = 21.5 Moles 'a 1/0.2 = 52.0 Moles'a 1/0.1 = 102.5 Moles 'a 1/0.1 = 103.0 Moles'a 1/0.1 = 10 The last three of the results are the same and that should not be the case which means that my results are not reliable and wrong. concentration Rounded average Rate of reaction in terms of 0.5 M 0.32's 3.131. Now i am going to draw a graph for rates and look how it goes up. I expect it not to be a best fit line because as I've already seen the results are not reliable. By doing this coursework and the experiment I found out that if you change concentration of the solution, to stronger the rate of the reaction will be a lot quicker than if i have a weaker concentrated solution.

I had some difficulties in doing the experiment because it was very hard to get everything right. On my preliminary, I didn't measure the volume of acid, so when I was doing my real experiment I knew I had to measure the acid. with my averages I don't I have any odd results. But I do have odds on my first experiment where I was measuring the time it took the gas to get to 5 cm 3. The odd result is when I used 2.0 Moles concentration and it took longer than 2.5 Moles, which is definitely not right.

2.5 Moles is more concentrated solution than 2.0 M. I did this experiment again but I changed what i was measuring, from 5 cm 3 to 10 cm 3 because the reactions happened to fast and my answers were not accurate. When I changed it. It was a lot easier to measure the volume of the gas and the answers were almost accurate. But when I drew my rate of reaction graph I saw that there is something wrong with my results.

One of the reasons for this may be that I got the odd answer for 2.5 Moles and that I was not accurate on measuring the time or the solution I have used was not properly concentrated. If I could do the experiment again I would increase the volume of the gas to 20 cm 3 and made sure that I would do the experiment couple of times. So I know that my results are more accurate..