### Conversion Guide for MeasurementsUse the following conversion factors to convert units:- **1 inch = 2.54 cm**- **1 kg = 2.20462 lb**- **1 mile = 1.61 km**Using these conversion factors and the International System of Units (SI) prefix, convert the following measurements to the desired unit. Ensure to maintain the precision of each measurement.#### Problems:a. Convert 12.34 inches to centimeters: - Given conversion factor: \(1 \text{ inch} = 2.54 \text{ cm}\) - Calculation: \[ 12.34 \text{ inches} = 12.34 \times 2.54 = 31.3436 \text{ cm} \]b. Convert 12.34 pounds to kilograms: - Given conversion factor: \(1 \text{ kg} = 2.20462 \text{ lb}\) - Calculation: \[ 12.34 \text{ lb} = \frac{12.34}{2.20462} = 5.5973298\text{ kg} \]c. Convert 12.34 meters per second to kilometers per hour: - Conversion factor for time: \(1 \text{ m/s} = 3.6 \text{ km/hr}\) - Calculation: \[ 12.34 \text{ m/s} = 12.34 \times 3.6 = 44.424 \text{ km/hr} \]### Answers:1. **Answer 1:** \[ 31.3436 \text{ cm} \]2. **Answer 2:** \[ 5.5973298 \text{ kg} \]

given 1 inch = 2.54 cm 1 kg = 2.20462 lb 1 mile = 1.61 km Also 1 hour = 3600 s so 1 s = 1/3600…

Use conversion factors below; • 1 inch = 2.54 cm • 1 kg = 2.20462 lb • 1 mile = 1.61 km and SI prefix, convert the following measurements to the desired unit. Be careful with the precision of each measurement. a. 12.34 inches = 31.3436 cm b. 12.34 Ib = 5.5973298 kg c. 12.34 m/s = 44.424 km/hr Answer 1: 31.3436 Answer 2: 5.5973298

Use conversion factors below; • 1 inch = 2.54 cm • 1 kg = 2.20462 lb • 1 mile = 1.61 km and SI prefix, convert the following measurements to the desired unit. Be careful with the precision of each measurement. a. 12.34 inches = 31.3436 cm b. 12.34 Ib = 5.5973298 kg c. 12.34 m/s = 44.424 km/hr Answer 1: 31.3436 Answer 2: 5.5973298

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

How many significant figures are in the following measurement: 0.00204 g Type your answer... Perform the following calculation. Enter the answer with the correct number of significant figure. 8.934+ 37.1 29 Be sure to start your answer with 0.xxxx, not just a decimal place, if appropriate. Ex. Enter 0.244 and NOT.244 Type your answer... Convert 69. kL to uL. Express your answer in scientific notation without writing units. Ex. 0.00222 is entered as 2.22*10^-3. Type your answer...
Carry out the following operations as if they were calculations fromexperimental data and express each answer in the correct units and with thecorrect number of significant figures.a. 5.6792 m + 0.6 m + 4.33 m =b. 3.70 g - 2.9133 g =c. 4.51 cm X 3.6666 cm =d. (22.4 g + 102.7 g + 0.005 g) / 5.478 ml =
The mass of a certain atom is 2.086 x 10°22 g. This is the same mass as 2.086 x 10-16 mg. 2.086 x 10-25 kg. 2.086 x 10-28 Hg. O 2.086 x 10-31 ng.
1.) There are exactly 2.54 centimeters in 1 inch. When using this conversion factor, how many significant figures are you limited to? A. unlimited number of significant figures B. depends on if you are using it in multiplication/division or addition/subtraction C. ambiguous D. 3 E. 1 2.)A room has dimensions of 10.0 ft × 20.0 ft × 8.00 ft. Given that there are three feet in a yard, what is the volume of the room in yd3? A. 178 B. 1.60 × 103 C. none of the above D. 59.3 E. 533 3.) What is the standard scientific form for the number 0.0002500? A. 2.500 x 104 B. 2.500 x 10-4 C. 2.50 x 10-4 D. 2.5 x 104
Conversions involving units raised to a power: include the correct number of significant digits. Follow the format example provided in the image. a. 4637 nm3 to in3
M Gmail YouTube = Maps O MEASUREMENT Counting significant digits when measurements are multiplied o... Multiply or divide the following measurements. Be sure each answer you enter contains the correct number of significant digits. 764.45 g 0.39 mL = 786.4 mol 48.853 L 7.81 mol L X 4.25 L = = 0 g mL mol 0- mol x10 X Ś 0/5 Olivi.
Question 2
Complete the following addition/subtraction calculations. Report your final answer to the correct number of significant figures and units. 14.62 g+ 0.1338 g 359.6+56.07 - 1088 367.2580 g - 80.4 g VI. Complete the following calculations. Report your final answer to the correct number of significant figures and units. 6.8 cm x 0.290 cm
Q.1. A student obtains the number 0.40076 on a balance. 4.00 x10 If this number actually has (3) significant figures, how should it be written? 0.400 0.4007 0.401 Q.2. Convert 5324 mL to m' (1000 L=1 m') 5.324 x10 5.324 5.324x10' 0.5324x10 Q.3. A student wants 25.0 g of acetone for a chemical 31.605 mL reaction. If the density of acetone is 0.791 g/mL, how many milliliters of acetone are needed? (take care about significant figures) 0.316 x10 19.7 19.77 Multiple optional
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