Lab Report 6 Dearing

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Apr 3, 2024

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Name: Eric Dearing College ID: 0550796 Thomas Edison State College General Chemistry I with Labs (CHE-121) Section no.: Semester and year: May 2014 LABORATORY REPORT Laboratory Assignment for Module 6: Gas Laws (eScience Lab 8) I. PURPOSE (10 POINTS) Explore concepts of Ideal Gas Law, Charles’ law, Boyle’s law, Gay-Lussac’s law, and the combined gas law. Utilize equations and mathematical theory gained from readings to calculate various measurements. II. TEST DATA (15 POINTS) Part 1: Ideal Gas Law—Finding Percent H 2 O 2 with Yeast Volume of O 2 collected: 0.058mL Total reaction time: 6min Temperature of water (in K): 294K Pressure (in atm): 0.04atm Volume of O 2 collected (in L) .058L Actual moles of O 2 collected 2.37 x 10 -3 Theoretical moles of O 2 (assume 100% H 2 O 2 density = 1.02 g/mL): 7.5 x 10 -2 1
Part 2: Charles’s Law—Effect on Temperature on Balloon Volume Temperatue, o C, of water (initial): 22C Circumference of balloon, cm (initial): 10cm Temperature, o C, of water (final): 84c Circumference of balloon, cm (final): 20cm III.CALCULATIONS (15 POINTS) Part 1: Ideal Gas Law—Finding Percent H 2 O 2 with Yeast Volume of O 2 collected: From 23mL mark to 81mL mark, 81-23=58mL O 2 collected Total reaction time: 2 minutes Temperature of water (in K): 21C + 273 = 294K Pressure (in atm): 753hpa / 760 = 0.99atm Volume of O 2 collected (in L) 58mL / 1000 = 0.058L Actual moles of O 2 collected n=PV/RT n=P(.99atm) V(0.058L) / R(0.0821) T(294K) = n 0.00237 or 2.37 x 10 -3 Theoretical moles of O 2 (assume 100% H 2 O 2 density = 1.02 g/mL): 5ml x 1.02g/ml x 1mol/34amu x ½ = .075mol O 2 IV.RESULTS (20 POINTS) Part 1: Ideal Gas Law—Finding Percent H 2 O 2 with Yeast Percent H2O2: 2.37 x 10 -3 x 7.5 x 10 -2 = 0.03 x 100 = 3% Reaction rate: 50ml / 120sec = 0.48 mL/sec Part 2: Charles’s Law—Effect on Temperature on Balloon Volume Temperature change: 22C to 84C = 62 degrees C increase Circumference change: 10cm to 20cm = 10cm increase 2
IV. CONCLUSION (10 POINTS) Using the Ideal Gas Law, and Charles’ law, I was able to calculate percent of H2O2 and view the effect of temperature on a balloons volume with Charles law. V. QUESTIONS (30 POINTS) Part 1: Ideal Gas Law—Finding Percent H 2 O 2 with Yeast 1. How does the calculated percentage of hydrogen peroxide compare to the label percentage (3%)? (6 points) Calculated percentage equals label percentage 2. Considering that catalysts are not consumed in a reaction, how do you think increasing the amount of catalyst would affect the reaction rate for the decomposition of hydrogen peroxide? (6 points) Increasing amount of catalyst would have no effect on this reaction due to the small amount of H2O2. However, if a greater amount of H2O2 was used a larger amount of catalyst would help speed the reaction. Part 2: Charles’s Law—Effect on Temperature on Balloon Volume 3. How does molecular motion of the air particles explain your results? Note that the pressure on the surface of the balloon remained constant, at atmospheric pressure. (6 points) While the atmospheric pressure outside the balloon remained constant, the molecular motion of air particles inside the balloon speeds up as the temperature increases. The faster molecules inside exert more force than the molecules outside. 4. What is another experiment, not listed in this manual, you could do that would demonstrate Charles’ law? Include the steps you would need to take in the procedure. (6 points) At room temperature, fill a balloon with air, measure circumference, place the balloon in a freezer for 10 minutes, re-measure circumference. 5. How do your results demonstrate Charles’s law? Use mathematical expressions to explain your answer. (6 points) As the temperature of the balloon decreases the circumference will decrease. Example: Room temperature T = 293K, circumference of balloon V = 40cm Freezer temperature T = 277K, circumference of balloon V = 20cm V/T = k, 40cm = V 300hpa / T 293 3
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