Chemistry Lab 1 Report
Experiment #: 1
Title: Chemical Kinetics
Purpose: Kinetics is the study of rates of reactions and how they
are influenced by certain factors like concentration, temperature.Two chemical tests were carried out. This was done to learn about how concentration and temperature influences the rate and figure out what the rate law order of reaction is.
Procedure:
Equation # 1: �2�3 2−(��) + 2�+( ��) → �(�) + �2��3(��) Prepare 5 tubes of different �2�3 2− with different volumes of solutions.
Test tube # 1: 10 mL of �2�3 2 add mix 10mL HCl and record
the reaction time. The solution became white, and cloudy after 33 seconds
Test tube # 2: 8 mL of �2�3 2 into the test tube with 2mL of
H2O and then mixed with 10 mL of HCI. The solution became white and somewhat cloudy after 45 seconds.
Test tube # 3: 6 mL of �2�3 2 into the test tube with 4mL of
H2O and then mixed with 10 mL of HCI. The solution became somewhat white and cloudy after 63 seconds.
Test tube # 4: 4 mL of �2�3 2 into the test tube with 6 mL of
H2O and then mixed with 10 mL of HCI. The solution became cloudy after 93 seconds
Test tube # 5: 2 mL of �2�3 2 into the test tube with 8 mL of
H2O and then mixed with 10 mL of HCI. The solution became cloudy after 191 seconds, had the least amount of reactant and was the most diluted.
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Equation # 2 2�2�2 → �2 (�) + 2�2� (�− is added through ��) Test how concentration and temperature affect rate, used a gas apparatus with three parts to measure the volume of O2. The three parts included a reaction chamber, with a stopper where we poured the reagent in. Next it is connected by a tube to this gas burette, the burette is graduated meaning it starts a 0 and goes on to 1,2,3, on downward to measure the volume of oxygen that’s produced next seeing the reaction it will find its way to the tube and its going to push the water down to the tube that is connected to the leveling bulb. If you take the stopper off and raise the leveling the green solution with go up and down the leveling bulb is used for atmospheric pressure. We will measure every 2 mins once the solutions have been mixed.
Trial # 1 (no temperature change): 5 mL of H2O2 was mixed with 10 mL
KI and15 mL of H2O. When KI was mixed into the solution, the solution turned yellow, and bubbles began to form and reached the 29.6 mL mark
after 3:06 minutes
Trial # 2: Doubled the volume to 10 mL of H2O2 was mixed with 10 mL KI
and keeping 10 mL of H2O the same. The KI was mixed into the solution, noticed that the rate increased almost doubled.
Trial # 3: Held the concentration of 5 mL of H2O2 was mixed with 20 mL
KI and 5 mL of H2O. Which also about doubled the rate of reaction.
Trial #4 (at 35 ℃): 5 mL of H2O2 was mixed with 10 mL KI and 15 mL of
H2O in heated water bath. Then KI was mixed into the solution, it turns yellow pretty quickly and then the timer was started after 2mL of gas is produced before starting the timer. Got at 30 ml after 53 seconds
Data/Results/Calculations:
�2�2/3−(��) + 2�+( ��) → �(�) + �2��3(��)
Test Tube Concentratio n w/HCL (M) Time (sec) Relative Rate (1 sec) 1 0.05 33 0.030
2 0.04 45 0.022
3 0.03 63 0.016
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