Measurement and Significant Figure Lab

Part 3: Calculate density of a metal an unknown metal. 1. Using the pictures below, record the displayed data in the data table in the report sheet. Make sure to include the right number of significant figures in the measurements and calculations. Mass measurement 7.1 g Volume of water measurement. There's only one measurement here – the larger image is for magnification only. -20 15 m Volume of water and metal measurement. There's only one measurement here – the larger image is for magnification only. 20 m 15

General Chemistry Laboratory I Lab 1 Significant Figures and Dimensional Analysis Student name PRE-LABORATORY QUESTIONS 1. How many significant figures are in each measurement? (1) 0.0044500 m (2) 5.003 km (4) 1.00 x 10³ s (5) 0.002 mm 2. Define accuracy and precision. 3. Convert 1.567 kilometers to centimeters.ccurate d 4. Convert 3.70 milligrams to kilograms. O Date: Page 1 IN-LABORATORY WORKSHEET 1. Give the number of significant figures in each of the following numbers. (1) 1,278.50 (2) 120,000 (4) 0.0053567 (5) 670 (7) 8.002 (8) 823.012 (10) 2.60 (Prepared by W. Song) (3) 10 dm (6) 10,000 m (3) 90,027.00 (6) 0.00730 (9) 0005789

Reflect on the importance of significant figures in measurements you have explored in this lab. In you summary: a. Briefly explain how you can use significant figures to address errors in measurements. b. Explain how you handle or account for significant figures in calculations i. Addition and subtraction ii. Multiplication and Division c. Describe how the skills obtained in this lab can be useful for a student pursuing a career in healthcare and provide some example scenarios.

2. Calculate the circumference. Diameter of watch glass was 10.2cm

I. Significant Figures and Conversion A. Scientific Notation 1. 58 cm → km 2. 67 W → MW 3. 196 mL L 4. 17 dm – cm 5. 299 W → TW

Expressing Errors in Measurement: Scientists often express their uncertainty and error in measurement by giving a percent error. The percent error is defined as: % error actual value - measured value x 100 actual value Answer the following four questions. Pay attention to significant figures, and show your work! 1. While doing a lab, a student found the density of a piece of pure aluminum to be 2.85 g/cm°. The accepted value for the density of aluminum is 2.70 g/cm³. What was the student's percent error? 22.70 26 Demystifying Scientific Data: RET 2006, Rev 2

What are the answers for the following questions?

For each of these problems, set up the calculation as described in your worksheet, using the proper conversion factor(s), and give the answer with the appropriate units and number of significant figures. Use scientific notation where appropriate. 1. Convert 5.89 inches into centimeters.

2. For this question you'll need to perform calculations for the data listed below. Imagine you performed the same set of measurements as the instructor did in the video using a 10-mL graduated cylinder. Be sure to show your calculations on this sheet. density of water 0.995124 g/ml mass of empty flask mass of flask + water 24.3165 g, 34.3175 g. 44.1982 g. 54.1597 g. 64.1712 g. 74.2704 g. 84.2420 g. 94.6730 g. 103.9727 g. 114.7728 g 15.5552 g (10 runs) a. Calculate the mean volume of water for the graduated cylinder data above. b. Calculate the standard deviation for the volume of water for the graduated cylinder data typed up above on this page. c. Calculate the standard error for the volume of water for the graduated cylinder data typed up above on this page.

Leaming Goal: To learn how to round an answer to the correct number of significant figures. Multiplication and division When multiplying or dividing, the final answer is rounded to the same number of significant figures as the measured number with the fewest significant figures. When we report a measurement in science, we are careful to report only digits known with certainty, plus a final digit that is recognized to be uncertain. We call this set of digits significant figures. Often, these numbers are used in calculations. When we use a calculator, the calculator does not automatically account for significant figures, so we have to do so ourselves. There are some basic rules for handling significant figures in calculations as shown in the table and outlined to the right. Addition and subtraction When adding or subtracting, the final answer is rounded to the same number of digits to the right of the decimal point as the measured number with the fewest digits to the right of the decimal…

1. Describe how to use conversion factors correctly using an example. 2. Write a number between 1.000 and 9999999.99. Write the number of significant figures in your number. 3. Give an example of how to find significant figures in calculations for A addition or subtraction B. multiplication and division

No need to explain. Just give the answers directly. Thank you. 1. Round off 1.274 to one (1) significant figure 2. Round off 1653 to one (1) significant figure 3. Round off 534.5 to three (3) significant figures

Which instrument would be used to measure the volume of a diamond? 1. graduated cylinder 2.triple-beam balance 3. Celsius thermometer 4. metric ruler

An electric current of 155.0 mA flows for 42.0 minutes. Calculate the amount of electric charge transported.. Be sure your answer has the correct unit symbol and 3 significant digits. 0 x10 μ 0 9 X

Convert 75 miles into meters. (Use the conversion 1.0 km = 0.621 miles and use metric conversions for the rest of the conversions).

Make a graph of the average mass vs. year. Make sure axes are labeled. Please please answer super fast please answer as fast as possible

It was still incorrect please solve it again.

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Determine which type of sampling technique is used. 19. A bread company wants to know whether men or women prefer their brand of bread so they randomly select from a group of men and a randomly select from a group of women for the sample. 20. Before leaving the room, the teacher asks students to write the number of hours they studied for the test on the chalkboard if they want to participate. 21. An electronics company wants to know which feature on one of their electronic devices is their customers' favorite. All customers who call technical support are surveyed. Choices for 19-28: A) Simple random sample B) Stratified sample C) Systematic sample D) Convenience sample E) Voluntary response sample 22. A corporation wants to know if its employees would rather work more days with less hours per week or less days with more hours per week. They randomly choose employees for the survey. 23. Brianna wants to figure out college students' thoughts about the availability of parking spaces on…

[Review Topics) [References) Use the References to access important values if needed for this question. A general chemistry student found a chunk of metal in the basement of a friend's house. To figure out what it was, she used the ideas just developed in class about density. She measured the mass of the metal to be 340.3 grams. Then she dropped the metal into a measuring cup and found that it displaced 15.7 mL of water. Calculate the density of the metal. Density = g/mL Densities of Some Common Substances Substance Density (g/mL) Water 1.00 Aluminum 2.72 Chromium 7.25 Nickel 8.91 Copper 8.94 Silver 10.50 Lead 11.34 Mercury 13.60 Gold 19.28 Tungsten 19.38 Platinum 21.46 This metal is most likely Submit Answer Retry Entire Group 9 more group attempts remaining Previous Email InstruC Cengage Learning | Cengage Technical Support W P. 63°F Mostly sunny DII PrtScn Home PgDn End F10 & R T. K L

(SHOW CALCULATIONS) The mass of a sample is 8.2 x 10-2 milligrams. Express that mass in kilograms with the proper number of significant figures. In your calculations, be sure to show the conversion factor.

PART 3 A Volumetric Flask + A С — ALI50 SOA A 50-mL volumetric flask measures a volume of 50.00 mL. In this experiment, we want to show that this is true. 50.00 mL is the actual volume measured by this volumetric flask. EXPERIMENT: The mass of an empty volumetric flask is measured. Then water is added to the volumetric flask and the meniscus is adjusted to be at the correct level. Then the mass of the volumetric flask and the water is measured. Finally, the temperature of the water in the volumetric flask is measured. RESULTS: Mass of empty volumetric flask = 37.04 g Mass of volumetric flask and water = 86.83 g Temperature of the water in the volumetric flask = 23°C 4 Densities of water at different temperatures: Density of Water at Different Temperatures (g/cm) Temp, °C Density Temp, °C Density Temp, °C Density 18 0.99862 21 0.99802 24 0.99733 19 0.99844 22 0.99780 25 0.99708 20 0.99823 23 0.99757 26 0.99681 (a) Using the mass of the water measured and the density of the water,…

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.

HOW TO GRAPH A CCA chemistry student needed to determine the % hexane in an unknown sample. The student determined density values for a set of standards and then measured the density value for the unknown sample. Using the experimental data from the student shown below, plot a line and determine % hexane for the unknown sample. You must also follow all the instructions given throughout this handout. % hexane 100.0 (SECTION 2) TO BE DONE BY HAND AND TURNED IN 80.0 60.0 40.0 20.0 unknown Density (g/mL) 0.642 0.684 0.724 0.766 0.806 0.699

I don't know how to do this. Please help.

QUESTION 20 A laboratory experiment was done at 160.0°F. Convert this temperature to Kusing the following equations and round appropriately. Give your answer with one digit after decimal. °C = (°F-32) x 5/9 K =°C + 273.15 Note that the conversions between Celsius, Fahrenheit, and Kelvin temperatures are exact. This means the fractions (5/9 or 9/5) and the numbers 32 and 273.15 are exact. So, use the addition/subtraction rule to determine the correct final answer. Directions: Type your answer only, no units.

2. While there were no calculations requi mbar conversions using dimensional analysis and still need to know how to do unit the proper number of significant figures. With that in mind, answer the questions below 1. How many significant figures are in each of the fol lowing quantities? a. 0.008 750 L 4 b. 3.40 x 10 m 2 c. 5 630 g 3 Si Convert 0.000 065 80 to scientific notation (without rounding). If a 6.00% (w/v) citric acid solution contains 6.00 grams of citric acid in every 100.0 mL of the solution, how many grams of citric acid are present in 385 mL of the 5.00% (w/v) solution? Show your work using dimensional analysis and report your answer with the correct number of significant figures. 3. 100AL %3D lo0g What volume of the 6.00% (w/v) citric acid solution described above would be needed to provide 425 mg of citric acid for a reaction? For full credit, show your work using a single dimensional analysis grid (or one chain of conversion factors) and report your answer with the…

Please answer question 12 part A

Please answer question number 2  correctly with the correct answer. there is a picture of an example of a ''Dimensional analysis Format' below. please write out all work showing the math in dimensional analysis format. (please show all work)   question 2: What is the mass of 1.00 mol of Oxygen (O2)?

What is the percent abundance (in units of percent) of zinc in a sample whose density is 7.639 g/mL and the only other component is copper? The density for pure copper is 8.96 g/cm³ and the density of pure zinc is 7.13 g/cm³. Report your answer to one decimal place. NOTE: This question is meant to give you practice before your data. The density value generated is random within a certain realistic constraint. It will not be representative of your data in the experiment.