and l x +zakeAssignment/takeCovalentActivity.do?locator-assignment-takeXA copy of your chemistry textbook is found to have a mass of 2.52 x 10³ grams. Using unit analysis, show what themass of the copy of your chemistry textbook is in milligrams.Use one of the following to set up the conversion factor.1 kg 1000 g1000 mL-1 L100 cm=1 m1000 mg=1 g1 mL=1 cm³1000 mm=1m32.52 x 10³ g x80F3EDSubmit AnswerC$4888F4RF(number) (unit)[Review Topics][References]Use the References to access important values if needed for this question.(number) (unit)%5VRetry Entire Group 8 more group attempts remainingCengage Learning Cengage Technical Support29F5TGA6BMacBook AirF6mgYH&7N44F7UJ* 008DIIF8IMK(9DDF9O<1)0LJF10]1000WP>.{Previous[114GNext>Save and Exit4))F12}* O1deleteMIT¡?Silift

Answered: Image /qna-images/answer/8f8aa467-c7ee-4e4f-8ce5-46417bccc25d.jpg

A copy of your chemistry textbook is found to have a mass of 2.52 x 10³ grams. Using unit analysis, show what the mass of the copy of your chemistry textbook is in milligrams. Use one of the following to set up the conversion factor. 1 kg=1000 g 1000 mL=1L 100 cm=1 m 1000 mg=1 g 1 mL=1 cm³ 1000 mm 1 m 2.52 x 10³ g x (number)(unit) Munit) mg

A copy of your chemistry textbook is found to have a mass of 2.52 x 10³ grams. Using unit analysis, show what the mass of the copy of your chemistry textbook is in milligrams. Use one of the following to set up the conversion factor. 1 kg=1000 g 1000 mL=1L 100 cm=1 m 1000 mg=1 g 1 mL=1 cm³ 1000 mm 1 m 2.52 x 10³ g x (number)(unit) Munit) mg

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

A chemist prepares a solution of nickel(II) chloride (NiCl₂) by measuring out 2.1 × 10² μmol of nickel(II) chloride into a 350. mL. volumetric flask and filling the flask to the mark with water. Calculate the concentration in μmol/L of the chemist's nickel(II) chloride solution. Round your answer to 2 significant digits. 0 μmol L x10
Given the following data, calculate the percentage of salt in the original mixture. Include the % unit and two decimal places in your answer. Mass of mixture = 4.578 g Mass of 400 mL beaker = 137.253 g Mass of 400 mL beaker and sand = 139.088 g Mass of 250 mL beaker = 105.77 g Mass of boiling chips = 0.548 g Mass of 250 mL beaker + boiling chips + salt = 108.834 g
Given the following data, calculate the percentage of salt in the original mixture. Include the % unit and two decimal places in your answer. Mass of mixture = 5.426 g Mass of 400 mL beaker = 137.521 g Mass of 400 mL beaker and sand = 139.477 g Mass of 250 mL beaker = 105.691 g Mass of boiling chips = 0.463 g Mass of 250 mL beaker + boiling chips + salt = 108.328 g
0.161 STARTING AMOUNT 0.161 km km + 10€ SHSSFE生 0.1 A city block is 0.161 km long. How many cm is this? 0.0161 0.000161 16100 161 0.001 0.00161 km 10 m 0.01 1 cm 1610 10€ 0.161 1000 100 16.1
A student uses a 100.00 mL volumetric flask to determine the density of a sample of water. The mass of the dry empty flask is determined to be 80.354 g. The flask is filled to the line 5 times with the water sample and the mass of the flask and the water is determined each time giving the 5 masses below. measurement 1: 172.275 g measurement 2: 172.288 g measurement 3: 172.28 g measurement 4: 172.263 g measurement 5: 172.378 g Based on the data given above, what is the average density of the sample in g/mL based on those measurements? Enter your answer with 3 significant figures.
4b. Convert the mass of the graduated cylinder with water using an analytical balance from grams to tons. 98.5107 g 4 4 13.8 mL 13.8 mL X 4 X 4 5. Beginning with the volume of water measured by the graduated cylinder, convert the volume from milliliters to liters and microliters. 4 4 4 P 4 15 15 L (rounded) HL 14 tons
You want to determine the density of a metallic solid object. The object weighs 144.38 grams. You a graduated cylinder where the water level is at 22.0 mL. The water level rises to 29.1l mL when you the cylinder. Calculate the density of the metal cylinder. 6. Mass of object = 7. Volume of object = 8. Density of object =
please see attached image
You have a stock solution certified by a manufacturer to contain 245.0 ± 0.4 µg SOź¯/mL. You would like to dilute it by a factor of 100 to obtain 2.450 µg/mL. Two possible methods of dilution are stated. For each method, calculate the resulting absolute uncertainty in concentration. Use the manufacturer's tolerances in the table for uncertainties. Glassware Tolerance 1-mL transfer pipet ±0.006 mL 10-mL transfer pipet +0.02 mL 100-mL volumetric flask +0.08 mL Method A: Dilute 10.00 mL up to 100 mL with a transfer pipet and volumetric flask. Then take 10.00 mL of the dilute solution and dilute it again to 100 mL. 0.0049 absolute uncertainty: ± ug/mL Incorrect Method B: Dilute 1.000 mL up to 100 mL with a transfer pipet and volumetric flask. 0.4 absolute uncertainty: ± ug/mL Incorrect
A chemist adds 35.0 mL of a 0.00187 mM copper(II) fluoride (CuF₂) solution to a reaction flask. Calculate the mass in micrograms of copper(II) fluoride the chemist has added to the flask. Be sure your answer has the correct number of significant digits. μg | x10
A nickel is found to have a mass of 4.87 grams. Using unit analysis, show what the mass of this nickel is in pounds. Use one of the following to set up the conversion factor. 454 g = 1 lb = 16 oz 1 m = 39.4 in= 3.28 feet 1 km = 0.621 mile 1 L = 1.06 qt 2.54 cm = 1 in 3.79 L=1 gal 4.87 grams X (number) 459 (number) lb Use the References to access important values if needed f g (unit) (unit) lb
I don't understand the wording. The least significant digit means the last digit? 7.700 X 2.1 = 16.17 would the uncertainty be 0.01 ? 2.132 + 17 + 4.04 = 23.172 would the uncertainty be 0.001 ?