A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g mL-1. The water temperature was 20 ° C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 mL of O2. (11) Calculate the percent error for the experiment. What is the observed molar volume? Moles of oxygen has been taken out now, molar volume at STP,volume of O2Vmmoles of 0245.1 ml of 020.00185 mole of O2IL1000 ml= 24. 37 LTo find out the percent error of this experiment:percent error =observed molar volumetheortical volumex 100х 10024.37 Y= 4. 10 X %

Given that,barometric pressure = 30.02 in Hg = 30.02 x 25.4 = 762.508 mm Hg1 in Hg = 25.4 mmHg Vapor…

Answered: A student performed the experiment…

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.105P

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A student performed the experiment described in this module, using 7.00 mL of a 1.8% H₂O₂ solution with a density of 1.01 g mL-1. The water temperature was 20 ° C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 mL of O₂.

(11) Calculate the percent error for the experiment.

What is the observed molar volume?

Moles of oxygen has been taken out now, molar volume at STP,
volume of O2
Vm
moles of 02
45.1 ml of 02
0.00185 mole of O2
IL
1000 ml
= 24. 37 L
To find out the percent error of this experiment:
percent error =
observed molar volume
theortical volume
x 100
х 100
24.37 Y
= 4. 10 X %

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