a. Calculate the following: (a) volumes (in cubic meters) of the tank in each trial (Hint: formula for volume cylinder = Tr²h, where r = radius, h = height), (b) mean of the volume, (c) standard deviation of the volume, and (d) CV of the volume b. Report the average volume of this cylindrical tank together with its uncertainty considering that its average radius is 2.70 ± 0.01 m.

a. Calculate the following: (a) volumes (in cubic meters) of the tank in each trial (Hint: formula for volume cylinder = Tr²h, where r = radius, h = height), (b) mean of the volume, (c) standard deviation of the volume, and (d) CV of the volume b. Report the average volume of this cylindrical tank together with its uncertainty considering that its average radius is 2.70 ± 0.01 m.

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

M Inbox (21,026) - sarahnasri522 × b Answered: Determine the mass X → C < + app.101edu.co Aktiv Chemistry X b Success Confirmation of Quest x Time's Up! 2 What is the mass percent of water in Ca(NO3)₂.4 H₂O? Provide an answer to two decimal places. G Google 1 4 7 +/- 5 x + 2 3 8 % 6 9 G 0 Submit X C x 100
Determine the Average Mass and the Standard Deviation for the following data: Mass of pennies in grams = 1.5021, 1.4736, 1.4966, 1.5164, 1.5420, 1.4699 g. Average Mass grams +/- Standard Deviation grams
Please don't provide handwritten solution .....
You receive an order for vancomycin 1850mg IV Q 6 H. Your institution carries pre-made IV bags of vancomycin 1000mg in 250 mL D5W in stock. a) How many bags of vancomycin 1000mg in 250 mL D5W will you need to pull from the shelf for one dose? b) How many mL of vancomycin 1000mg in 250 mL D5W will you need to discard to provide the patient with their dose?
Student B determined the density of water to be 1.04 ± 0.05 g/mL. Consider Students A results. Which student was more accurate? Which student was more precise? (Student A got the following densities of water; 1.09 g/mL, 1.14 g/mL, and 1.15 g/mL with an average of 1.127 g/mL and a standard deviation of 0.026 g/mL)
What is the empirical formula of copper chloride for this lab?
What is the absolute uncertainty and relative uncertainty of the molarity of the solution? M = = 0.078376462 = 0.078 M Pb2+
1
Julie has been asked to measure the concentration of a sample solution using a spectrophotometer. After a first attempt, she realizes that, to make the measurement, she must first dilute the sample solution. Julie transfers 2.3 mL2.3 mL of the sample to a 250 mL250 mL volumetric flask and fills the rest of the flask with water to the 250 mL250 mL line. She then uses the spectrophotometer to measure the concentration of the dilute solution as 5.5×10−5 M.5.5×10−5 M. What is the concentration of the starting sample solution? sample solution concentration: M
The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μLμL of the sample and injecting it into a cuvette already containing 2.00 mLmL of water (total volume is 2.00 mLmL + 100.0 μLμL). The absorbance value of the diluted solution corresponded to a concentration of 7.71×10−6 M M . What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units.
To prepare a solution of KCl, you weigh out 1.5672 (± 0.0003) g and dissolve it in a volumetric flask of 250.00 (±0.50) mL in volume. Express the molarity of the solution and its uncertainty with appropriate number of significant figures. (Formula mass of KCl is 74.551 ± 0.004 g/mol)
Please type answer note write by hend.