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Investigation into the Rate of Reaction between Calcium Carbonate and Hydrochloric Acid.

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Introduction

Ali Rana 11MW Investigation into the Rate of Reaction between Calcium Carbonate and Hydrochloric Acid. The reaction which I will be investigating is: Calcium Carbonate + Hydrochloric acid Calcium Chloride + Water + Carbon Dioxide CaCo3 (s) + HCL (aq) CaCl2 (aq) + H20 (l) + CO2 (g) Aim I have decided to investigate into the effect of different concentrations of hydrochloric acid on calcium carbonate. Plan I want to see how much Carbon Dioxide is given off after 60 seconds, once the acid and marble start reacting. I carried out a preliminary experiment to see what sort of time ranges I was going to expect because I wanted to get the concentration levels right otherwise I could have been waiting for a long time. In this investigation I will be using the following apparatus; one conical flask to put the marble powder in and also to put the acid in so they react. A 50ml measuring cylinder to measure the amount of acid and water to make my acid concentrations. I will need a gas syringe to measure how much gas is being given off and a stop watch. I will also need one balance to measure the weight of the calcium carbonate powder. ...read more.

Middle

For example, a mixture of iron and sulphur is heated in a Bunsen burner flame, the mixture starts to glow. The glow spreads through the mixture, even if the flame is removed. This is because, energy is being given out. So, I predict that as the concentration of acid decreases there will be fewer effective collisions between the acid and calcium carbonate. Results Test 1 10 20 30 40 50 60 23 43 52 60 62 67 21 30 42 46 47 54 16 22 25 29 32 32 7 10 13 14 14 14 4 4 5 6 6 7 Time (secs) Concentration (ml) HCL/ H2O 50/ 0 40/ 10 30/ 20 20/ 30 10/ 40 Test 2 10 20 30 40 50 60 27 42 54 63 64 69 18 29 41 46 47 54 15 18 27 28 31 32 9 10 14 16 17 17 2 5 5 5 5 5 Time (secs) Concentration (ml) HCL/ H2O 50/ 0 40/ 10 30/ 20 20/ 30 10/ 40 Test 3 10 20 30 40 50 60 25 44 47 58 62 68 22 31 45 48 53 54 17 19 32 33 35 36 8 10 13 15 15 15 3 8 8 8 8 8 Time (secs) ...read more.

Conclusion

I have already mentioned the problem of the gas having to push itself up the delivery tube before it was collected. This added time onto the true time taken. This means my results are higher then they should be. The truth of my conclusion is not undermined by this however, as the same effect happened to each test. I could overcome this problem and the one mentioned before by only starting the timer when the gas starts to fill the measuring cylinder. This would not include the time taken to push the gas up the delivery tube in my results, and I would not have to start the stopwatch at the same time as putting the acid in the flask. To provide more evidence for my investigation I could use a thermometer to measure the temperature during the experiment, this would show whether my theory of the lower concentration not heating up the reactants is true or not. For further investigation, I could use stronger acid to see if there is a limit to how quickly the reaction can take place. Also, I could measure the mass loss of the reaction by having the conical flask on a top pan balance. I could take away the mass at regular intervals from the original and find out how quickly the reaction takes place. ...read more.

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