How Temperature Is Able To Affect Chemical Reaction’s Rate Between Hydrochloric Acid And Calcium Carbonate
Table of Contents
It is suggested that
Materials:
Process
Observations générales
Calculations:
Conclusions and Evaluation
A supposition or possible explanation that can be tested by further investigation.
Temperature increases will result in a faster rate of reaction because the molecules have more kinetic energies and can easily overcome the activation.
Independent Variable: Temperature
Dependent variable: product produced at a specific time
Constants: time, concentration
Materials:
Electric Stove Top
Hydrochloric Acid (1 mol)
Calcium Carbonate
Cylinder with a capacity of +-0.1 milliliters
Halt
Timer +-0.1 s
Temperature gauge accurate to within 0.1 C
Tube Stopper
Clamp
Beaker of 0.1 ml
Water
Flask
Scale +-0.1g
Process
Fill up the cylinder.
Fill 2000 ml of water into the beaker.
Turn the cylinder upside down and pour the water in the 2000ml Beaker.
Clip the odometer to the ringstand about 2 inches from the bottom.
Have the stopper and tube ready.
6Measure and dilution 5 ml (1 mole) hydrochloric in 80ml water. Fill the beaker.
If not, place the beaker on the hot plate to heat it up. If not, place the beaker onto the hotplate to bring it up to temperature.
Take 1 g Calcium Carbonate.
Fill up the flasks with Calcium Carbonate
Start the timer and fill the flask up with hydrochloric. Stopper the flask quickly.
Holding the flask, gently stirr it for 4 min.
After recording the 4 minute displacement, the distance made is recorded.
Step 7 is the same for all the other variables (32degC), 43degC (for the next four), 52degC (for the fifth variable), and 62degC (for the sixth). Be sure to heat the food to the correct temperature.
Observations générales
The temperature was difficult to maintain
You will get different amounts of gas each time you stir.
Gas was lost because the stopper had to be activated faster. The stopper could not be turned on instantly with both reactants.
Calcium Carbonate stucks to the container.
The amount of gas produced was related to the temperature change.
Calculations: The balance equation
CaCO3(s) + 2 HCl(aq) = CaCl2(aq) + CO2(g) + H2O(l)
(Using variable 1): Trials: 5.7 ml, 5.9 ml, 6.0 ml
Add all the numbers together: 5.7 + 6.9 + 5.9 = 17.6
Divide 17.6 by 3 to get 5.9
Conclusion and evaluation:Overall, the data I collected supports my hypothesis. The temperature and amount of gas produced were correlated. The gas production increases as the temperature rises because reactions take place at a quicker rate. The experiment was full of errors. For example, gas was lost. It was due to the time it took to pour HCL into flasks and to apply the stopper. The results were inaccurate because gas was lost to the exterior and we could not measure it. However, the final results were similar. On the graph, the percentage increase is low. However, as we reach 52degC the percentage increases. The activation energies are overcome around the 42-52deg C temperature range. Therefore, the gas produced in the 52-62deg C zone is much greater than that of the 22-42deg C zone. The temperature fluctuates, and I’m not able get the perfect temperature for every experiment.
The entire set-up takes a lot more time than I thought. The hardest part was trying to turn the cylinder over without losing any water. Another problem was pouring HCL with Calcium Carbonate inside the flask then closing the lid. As I explained before, this was causing gas to escape and cause inaccurate data. The stirring was another issue. Every experiment I’ve done, the rate of stirring is different. This is my fault.
The experiment has many limitations. One of them is the instrumentation used. Due to the instruments, it was difficult to achieve the desired precision. Also, the temperature fluctuated and was difficult to control. For this experiment to be improved, I will need more precise instruments. You should also find a method to prevent water from being lost when you turn the cylinder upside-down.
