A certain analytical method for the determination of lead yields masses for lead that are low by 0.4 g. Calculate the percentrelative error caused by this deviation for each measured mass of lead. Report the percent relative error with the correct numberof significant figures.872.4 g lead:-0.04% relative error107.6 g lead:-0.3% relative error70.6 g lead:-0.5% relative error山T回hulustv

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Answered: relative error caused by this deviation…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter5: Errors In Chemical Analyses

Section: Chapter Questions

Problem 5.8QAP

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The density of an irregularly shaped object was determined as follows. The mass of the object was found to be 28.90 g 0.03 g. A graduated cylinder was partially filled with water. The reading of the level of the water was 6.4 cm3 0.1 cm3. The object was dropped in the cylinder, and the level of the water rose to 9.8 cm3 0.1 cm3. What is the density of the object with appropriate error limits? (See Appendix 1.5.)
Hexane (C6H14, density = 0.766 g/cm3), perfluoro-hexane (C6F14, density = 1.669 g/cm3), and water are immiscible liquids; that is, they do not dissolve in one another. You place 10 mL of each in a graduated cylinder, along with pieces of high-density polyethylene (HDPE, density = 0.97 g/cm3), polyvinyl chloride(PVC, density = 1.36 g/cm3), and Teflon (density = 2.3 g/cm3). None of these common plastics dissolves in these liquids. Describe what you expect to see.
What are the steps in the Chapman cycle? Explain the importance.
If you repeat the same measurement many times, will you always obtain exactly the same result? Why or why not? What factors influence the repeatability of a measurement?
Two students were assigned to determine the mass of a sample of an unknown liquid. Student A used an ordinary laboratory balance that could determine mass to ±0.01 g. Student B used an analytical balance that could measure mass to ±0.1 mg. Each made four measurements, giving the following results: Student A: 8.19 g, 8.22 g, 8.21 g, 8.25 g Student B: 8.2210 g, 8.2210 g, 8.2209 g, 8.2210 g 2. Which student is more precise? A B
Many times errors are expressed in terms of percentage. The percent error is die absolute value of the difference of the true value and the experimental value, divided by the true value, and multiplied by 100. Percenterror=truevalue-experimentalvaluetruevalue100 Calculate the percent error for the following measurements. a. The density of an aluminum block determined in an experiment was 2.64 g/cm3. (True value 2.70 g/cm3.) b. The experimental determination of iron in iron ore was 16.48%. (True value 16.12%.) c. A balance measured the mass of a 1.000-g standard as 0.9981 g.

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