Your laboratory instructor has given you two metal cylinders. The mass of each sample was determined on a balance to five significant figures. The volume was determined by (a) measuring the dimensions of the cylinders and (b) immersing the samples in a graduated cylinder as shown in the figure below. The initial volume of water was 25.0 mL. The uncertainty of the volume measurement using the graduated cylinder is +/-0.1 mL. Cylinder A Cylinder B 40 40 30 30 20 20 10 10 Mass (g) Height (cm) Diameter (cm) Cylinder A 15.560 5.11 1.20 Cylinder B 35.536 5.90 1.30 Which statements are true about the number of significant figures in the volume measurements? The dimension method volume has one significant figure. The dimension method volume has two significant figures. The dimension method volume has three significant figures. The water displacement volume has one significant figure. The water displacement volume has two significant figures. The water displacement volume has three significant figures. 000000

Your laboratory instructor has given you two metal cylinders. The mass of each sample was determined on a balance to five significant figures. The volume was determined by (a) measuring the dimensions of the cylinders and (b) immersing the samples in a graduated cylinder as shown in the figure below. The initial volume of water was 25.0 mL. The uncertainty of the volume measurement using the graduated cylinder is +/-0.1 mL. Cylinder A Cylinder B 40 40 30 30 20 20 10 10 Mass (g) Height (cm) Diameter (cm) Cylinder A 15.560 5.11 1.20 Cylinder B 35.536 5.90 1.30 Which statements are true about the number of significant figures in the volume measurements? The dimension method volume has one significant figure. The dimension method volume has two significant figures. The dimension method volume has three significant figures. The water displacement volume has one significant figure. The water displacement volume has two significant figures. The water displacement volume has three significant figures. 000000

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter1: Basic Concepts Of Chemistry

Section: Chapter Questions

Problem 21RPS: You and your lab partner are asked to determine the density of an aluminum bar. The mass is known...

See similar textbooks

Similar questions

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.)
A student checked the accuracy of two standard top-loading balances by testing them with a standard 5.000-g mass. The results were as follows: Balance 1: 4.99 g, 5.04 g, 5.03 g, 5.01 g Balance 2: 4.97 g, 4.99 g, 4.95 g, 4.96 g Calculate the average values for balances 1 and 2 and calculate the percent error for each. Which balance is more accurate?
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.
A sample of a bright blue mineral was weighed in air, then weighed again while suspended in water. An object is buoyed up by the mass of the fluid displaced by the object. In air, the mineral weighed 7.35 g; in water, it weighed 5.40 g. The densities of air and water are 1.205 g/L and 0.9982 g/cm3, respectively. What is the density of the mineral?
Express the following measured values in scientific notation to the correct number of significant figures. a. 120.7 b. 0.0034 c. 231.00 d. 23,100
Suppose you were measuring out an organic liquid, and some of it is evaporated after you have performed the volumetric measurement while you are weighing out the sample. What effect would this have on the densities you calculated? Will you overestimate or underestimate the density of the liquid? Would this cause poor accuracy, low precision, or both? Explain briefly.
A.Measurement of the density of water.Weigh a small beaker (degree of precision?). Place about 25 mL of water in a 50 mL graduated cylinder and record its volume (degree of precision?). Pour the water into the beaker and weigh the beaker and water together. From these data, calculate the density of the water, giving your answer with the proper number of significant figures.Volume of water in cylinder23.5 mLMass of empty beaker75.360 gMass of beaker with water 99.030 gMass of water in beaker ______gDensity of water g/mL
The pharmacist attempts to weigh 0.375 g o morphine sulfate on a balance of dubious accuracy. When checked on a highly accurate balance, the weight is found to be 0.400 g. Calculate the percentage of error in the first weighing.
We did an experiment about the density of a lead sinker and the thickness of the aluminum foil. We used water displacement to measure the volume of the lead sinker (using a graduated cylinder) and we used a ruler for the measurement of the length and width of the foil and analytical balance for the mass. The result of the experiment does not follow theoretical data. According to the RSC, Lead has a density of 11.3 g/cm3, but after calculating the result of the experiment we gathered around 9.3 g/cm3. Furthermore, according to others' experiments, the thickness of their aluminum foil is around 0.00027 cm while based on the result of our experiment, the thickness is about 0.0013 cm. My questions are: In density, since it is an intensive property, the result should be 11.3 g/cm3. However, the result of our experiment was different from the theoretical data. The reasoning is correct, right? The result of the experiment should be 11.3 g/cm3. If it is not then we had committed an error in…
A student has been given a solid sample and asked to calculate its density. She measured the mass of the solid sample and recorded it on her data sheet as 4.528g. she recorded the intital volume as 4.7 mL and a final volume as 6.2mL. What is the density of the sample?
In order to find the density of a solution of unknown density, 10 mL of solution was drawn into a clean and dry beaker three times with a pipette and weighed and the weighing results were found to be 65.1452 g, 64.9982 g, 65.1027 g. Calculate the density of the solution and the standard deviation of the measurements, since the empty weight of the beaker is 52.2461 g.
A sample of metal pellets weighs 13.54 g. When this sample was placed in a 100-mL graduated cylinder, which contained 25.5 mL water, the new volume (of water and pellets combined) was 27.0 mL. If the metal is one of the solids listed in Table 1, what is the identity of the metal? Show your calculations and use the correct rules for determining significant figures in calculations as shown in the background section. Explain your identification.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS