IndexHypothesisMaterials:ProcedureGeneral observations:Calculations:Conclusion and evaluation:HypothesisIf the temperature increases, the reaction rate between the reactants will increase because the molecules will gain more kinetic energy and be easier to overcome the activation energy. Say no to plagiarism. Get a tailor-made essay on "Why Violent Video Games Shouldn't Be Banned"? Get an original assayIndependent variable: temperatureDependent variable: product made in a fixed timeConstants: time, concentrationMaterials: hot platehydrochloric acid (1 mol)calcium carbonateCylinder ±0.1 mlCapTimer ±0.1 secThermometer ±0.1 CCap tubeClamp 0. 1mlWaterFlaskScale ±0.1gProcedureFill the cylinder with water.Fill the 2000ml beaker with water.Invert the cylinder upside down, without losing water, into the 2000ml beaker.Secure the odometer approximately 2 inches above the bottom of the beaker on the stand ring.Place the tube inside the cylinder and keep the stopper ready for the flask.6Measure 5 ml of 1 mole hydrochloric acid and dilute it in 80 ml of water and fill the glass.Check whether the hydrochloric acid is present with the thermometer. it is at room temperature (22° C). If not, place the glass on the hot plate to heat it to the right temperature. Measure 1 g of calcium carbonate. Fill the flask with calcium carbonate Fill the flask with hydrochloric acid and start the timer. Quickly close the flask. Hold the flask and shake lightly for 4 minutes. After 4 minutes, record the movement made. For the rest of the variables (32° C, 43° C, 52° C and 62° C), repeat the steps 3-12 but in step 7. Make sure you heat it to the right temperature. General observations: The temperature was difficult to keep constant. If you mix differently each time, the amount of gas produced varies with each trial. Some gas was lost inserting both calcium carbonate and hydrochloric acid because the cap needs to be inserted more quickly. There was no way to instantly close the cap with both reagents. The calcium carbonate stuck to the container it was placed on. There was a correlation between the amount of gas produced and the change in temperature. Calculations: The balanced equation: CaCO3(s) + 2 HCl(aq) = CaCl2(aq) + CO2(g) + H2O(l)(Using variable 1): Tests: 5.7 ml, 5.9 ml , 6.0 ml Add them all together: 5.7 + 6.0 + 5.9 = 17.6 Then divide it by 3: 17.6 / 3 = 5.9 Conclusion and evaluation: Overall, my data supports the 'hypothesis I made. There was a correlation between temperature and the amount of gas produced. As the temperature increases, the amount of gas produced increases because the reactions occur at a faster rate. There were many random errors in this experiment, such as gas lost during the experiment. The reason was that the amount of time it takes to pour the HCL into the flask and also the amount of time to put the cap on makes the results inaccurate, because the gas is lost outside and we can't measure it, but in the end you have again similar results. In the graph you can see that the percentage of increase was low but when we reach 52° C the percentage becomes higher. I believe that around the 42 – 52°C range the temperature is high enough to overcome the activation energy, that's why the gas produced is much higher in the 52 – 62°C range than at the true 22 – 42°C. The systematic error in this experiment is the temperature, because the temperature fluctuates as I can't get the perfect temperature with every experiment. I think the procedure was followed very well, but the whole setup takes a long time. The hardest part of the experiment was turning the cylinder over without trying,.