How can we speed up the reaction between Calcium Carbonate and Hydrochloric Acid? Contents 1. Plan Aim Equipment Variable Factors Prediction Method Trial Run 2. Results Results Tables 3. Analysis and Conclusions Graphs Conclusions 4. Evaluation Accuracy Of Results Reliability Improvements Extending the Investigation 1.
PlanA imI am doing this experiment to find out how I can speed up the reaction rate between calcium carbonate and hydrochloric acid. Equipment This is the equipment I will use: Gas Syringe Glass Flask Calcium Carbonate hydrochloric acid Variable Factors The factors that could slow down or speed up this reaction are: The size of the Calcium Carbonate (marble) pieces – This will affect how fast the acid reacts with the marble, the smaller the pieces, the bigger the surface area so the reaction can take place faster. The amount of Calcium Carbonate – The more calcium carbonate there is, the more carbon dioxide will be produced and the larger the reaction will be. The amount of Hydrochloric Acid – The more hydrochloric acid there is, the more carbon dioxide will be produced and the larger the reaction will be. The temperature of the materials – The temperature of the materials determines how fast the reaction will take place. The hotter the materials, the faster the reaction and vice-versa.
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During my experiment, I have been investigating my research question: To what extent do white and brown eggshells differ in respect to percentage by mass of calcium carbonate content? Calcium carbonate is a substance found in the eggshells giving them hardness and strength. It is essential to the commercial egg industry that the biggest possible amount of eggs reaches the market. Hence, as calcium ...
The concentration of Hydrochloric Acid – The higher the concentration (strength) of the acid, the faster it will react. The purity of the Calcium Carbonate pieces – The purity of the calcium carbonate will affect the speed of the reaction also. Prediction From previous experiments I have learned that if large pieces are broken into smaller pieces they react faster because they have more surface area. This is because at the molecular level, there are more molecules at the surface of the chips for the molecules of acid to react with when the chips are broken into smaller pieces. The same principle can be applied to the marble chips. The smaller the chips the more surface area so I predict that the smaller marble chips will react faster than the larger chips.
Method Here is the set up: In this experiment I will be keeping the variables I mentioned earlier the same except one to keep the experiment fair. I will be changing the size of the marble chips to see which size reacts the fastest. The gas syringe is firstly clamped to the stand and a plastic tube and bung are attached to the syringe. The marble chips are then measured out (I will be using 2 g of marble chips each time) and the hydrochloric acid (10 ml) is added to the flask.
The chips are then added and the bung is quickly placed over the flask to create an airtight seal. The amount of carbon dioxide in the gas syringe is read off every 10 seconds until the reaction stops or the gas syringe runs out of capacity (100 ml).
Risk Assessment Goggles must be worn at all times to prevent acid going in eyes. Gas syringes must be handled with care to prevent accidents Variables Table Dependant Variable Value How Measured Amount of carbon dioxide collected Amount read every 10 seconds. 2 repeats for each size of marble chip Gas syringe and digital stopwatch Independant Variable Size of marble chips Powder, small, medium and large chips prepared by teacher. 2 g used each time.
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Size measured by third party. Weighed using digital scales. Control Variables Amount of acid 10 ml each time Measuring Cylinder Concentration of acid 1 molar acid Measured by third party. Temperature Room temp. Approx 27 C N/Purity of calcium carbonate Assumed the same purity Same batch used each time Trial Run Time (sec) Powder (ml of CO) Small (ml of CO) Medium (ml of CO) Large (ml of CO) 10 44 7 8 220 68 13 10 230 79 24 23 240 91 29 32 250 100 35 39 260 42 47 270 53 53 280 61 61 290 70 67 2100 79 72 2110 84 75 2120 100 80 2130 84 2140 89 2150 93 2160 97 2170 100 2 These trial run results helped me with my final method 2. Results Time (sec) Amount of Carbon Dioxide (ml) Powder (ml of CO) Small (ml of CO) Medium (ml of CO) Large (ml of CO) 10 59 75 8 10 11 14 5 320 73 92 14 16 17 21 5 330 83 96 21 24 23 30 5 340 92 100 30 34 30 38 5 350 100 40 44 36 46 5 360 50 53 42 55 5 370 59 62 49 62 5 380 69 71 55 69 5 390 76 78 62 74 5 3100 84 86 67 82 5 3110 91 92 72 86 5 3120 97 98 76 91 5 3130 100 100 80 97 5 3140 85 100 5 3150 90 5 3160 95 5 3170 97 5 3180 100 5 3 Control variables Amount of Hydrochloric Acid = 10 ml Amount of Calcium Carbonate = 2 temperature = Approx.
27 Acid Concentration = 1 molar 3. Analysis and ConclusionsGraphsConclusionBy looking at the results table and the graph, I am able to prove my predictions correct. The smaller the size of marble chip, the faster it will react with the acid. This is because there is a bigger surface area meaning a larger surface for the acid to react with. The large marble chips in my experiment only reacted with the acid on the outside of the chip and there was un reacted marble inside because the acid couldn’t reach it. As the marble chips got larger, the reaction with acid was slowed until the size of the chips reached a point where they only reacted with the outside of the marble.
I think once it gets to this point, it does not matter about the size of the marble chips anymore because they will only react with the surface of the marble and not penetrate the inside. 5. Evaluation Accuracy of results There is always some degree of inaccuracy in any experiment. I think that there were several factors in my experiment that made the results slightly inaccurate. These were; The time taken to place the bung on the flask – This let out a small amount of carbon dioxide into the atmosphere instead of the gas syringe. Weighing and measuring inaccuracy’s – The weighing of the marble chips will always be slightly inaccurate due to the scales inaccuracy.
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... the rate of reaction making my results less accurate. Although the marble chips were roughly the same size they weren’t all exactly the same ... means that there is very little chance of acid particles colliding with the marble chip with enough energy to react. In a high ... feel this problem is major as the variations were relatively small as is shown by the error margins drawn on my ...
This is the same with the measuring of acid. The size of the marble chips – The size of the marble chips was not always the same, some were larger or smaller than others. This would have made for a slight inaccuracy. Reliability No significant problems or difficulties were encountered when carrying out this experiment. The accuracy and reliability of the results and conclusions are very good. Even though I have outlined the inaccuracy’s of the experiment, these are only t be expected and do not have much impact on the overall conclusion.
Improvements The procedure used was simple and straightforward and not many difficulties were encountered. One difficulty was that the gas syringe was subject to humidity which made the syringe move not as smoothly as it would have otherwise. A small improvement could be made to the method of mixing the marble and acid as a small amount of gas was wasted when securing the bung onto the flask. There could also be slight improvements made with respects to the accuracy of the equipment used. Extending the investigation If I had wanted to investigate further, I would have changed the different control variables to see which combination gave the fastest reaction time. I would of also tried different sizes of chips measured exactly with a bigger range of sizes.
It would also be interesting to add a catalyst to the reaction or to use a different atmosphere in the flask such as nitrogen or helium.
