Compare The Rate Of Reaction Between Aceic Acid And Acetic Acid
Hypothesis: If I increase the concentration of NaOH from 0.5M to 1M, then I will see the temperature slope increase in the reaction with an increased concentration because with an increase of moles, the particles will be colliding more often, therefore increasing the probability that the proper energy and alignment will occur to create more collisions in the same amount of time.
Methods: List of Materials:
• 110 mL of NaOH at 1 M (10 mL per run)
• 110 mL of NaOH at 0.5 M (10 mL per run)
• 220 mL of Acetic Acid at 50% (10 mL per run).
• Vernier Temperature Probe.
• Erlenmeyer Flask 200 mL.
• Graduated Cylinder 25 mL.
• Charged Computer with LoggerPro.
Method: I gathered all my materials along with obtaining a lab coat, safety glasses, …show more content…
This graph shows the exothermic reaction of 10 mL of NaOH at 0.5M with 10 mL of Acetic Acid at 50% and the temperature change per run. The NaOH at 0.5M produced a lower temperature change as it had a lower concentration than the NaOH at 1M.
Conclusions: I accept my hypothesis that the NaOH at 1.0 will caused a greater exothermic reaction with the Acetic Acid at 50% as a higher concentration will cause a reaction rate to increase faster. I know the data supports the rate of reaction theory because, Graph #1 shows an increase in temperature from an average reactants temperature of 21.09 °C to an average activated complex temperature of 22.39 °C. This is a support piece of evidence that increase in concentration of an acid will cause the rate of reaction itself to expedite.
Evaluation: By making my controlled variable stay at a reliable measurement of 10 mL each time will insure that my results remain reliable. An example is not having access to NaOH at 0.5M therefore having to create my own through diluting 5 mL of NaOH with 5 mL of distilled water. This was an inaccurate way to test NaOH at 0.5M since there was no way of demonstrating that the 10 mL of liquid in the Graduated Cylinder is for sure the NaOH at 0.5M. For future experiments, I would design a procedure which would use materials I know to be fully
Methods: List of Materials:
• 110 mL of NaOH at 1 M (10 mL per run)
• 110 mL of NaOH at 0.5 M (10 mL per run)
• 220 mL of Acetic Acid at 50% (10 mL per run).
• Vernier Temperature Probe.
• Erlenmeyer Flask 200 mL.
• Graduated Cylinder 25 mL.
• Charged Computer with LoggerPro.
Method: I gathered all my materials along with obtaining a lab coat, safety glasses, …show more content…
This graph shows the exothermic reaction of 10 mL of NaOH at 0.5M with 10 mL of Acetic Acid at 50% and the temperature change per run. The NaOH at 0.5M produced a lower temperature change as it had a lower concentration than the NaOH at 1M.
Conclusions: I accept my hypothesis that the NaOH at 1.0 will caused a greater exothermic reaction with the Acetic Acid at 50% as a higher concentration will cause a reaction rate to increase faster. I know the data supports the rate of reaction theory because, Graph #1 shows an increase in temperature from an average reactants temperature of 21.09 °C to an average activated complex temperature of 22.39 °C. This is a support piece of evidence that increase in concentration of an acid will cause the rate of reaction itself to expedite.
Evaluation: By making my controlled variable stay at a reliable measurement of 10 mL each time will insure that my results remain reliable. An example is not having access to NaOH at 0.5M therefore having to create my own through diluting 5 mL of NaOH with 5 mL of distilled water. This was an inaccurate way to test NaOH at 0.5M since there was no way of demonstrating that the 10 mL of liquid in the Graduated Cylinder is for sure the NaOH at 0.5M. For future experiments, I would design a procedure which would use materials I know to be fully