Lab Report 6 Dearing

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Thomas Edison State College *

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121

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Chemistry

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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
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