Chemistry Lab
Mecky18
CHM101LM6IdealGasLawConstantLabReport.docxDetermination of Ideal Gas Law Constant Student Name Date
Data
Activity 1
Data Table 1
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Trial 1 (1 mL H2O2) |
Trial 2 (1 mL H2O2) |
Trial 3 (2 mL H2O2) |
Trial 4 (2 mL H2O2) |
Trial 5 (3 mL H2O2) |
Trial 6 (3 mL H2O2) |
Trial 7 (4 mL H2O2) |
Trial 8 (4 mL H2O2) |
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Air temperature (°C) |
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Volume H2O2 liquid (mL) |
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Initial Volume Gas (mL) |
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Final Volume Gas (mL) |
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ΔV (mL) |
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Would the volume of oxygen that is generated be affected if a smaller mass of yeast were used? Why or why not?
Activity 2
Data Table 2
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Concentration H2O2 (mol/L) |
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Trial 1 (1 mL H2O2) |
Trial 2 (1 mL H2O2) |
Trial 3 (2 mL H2O2) |
Trial 4 (2 mL H2O2) |
Trial 5 (3 mL H2O2) |
Trial 6 (3 mL H2O2) |
Trial 7 (4 mL H2O2) |
Trial 8 (4 mL H2O2) |
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Moles H2O2 |
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Moles O2 |
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ΔV (L) |
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*Hint: Use stoichiometry to solve for moles of O2.
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Air Temperature (K) |
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Air Pressure (atm) |
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Equation of the Line |
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Gas Constant R |
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Percent Error |
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Identify at least two potential sources of error in the experiment. Are any assumptions made that would add to the experimental error?
