Units of measurement
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This document discusses units of measurement and standards used in chemistry. It covers tools used to measure length, volume, time, weight, temperature. The US customary and metric systems are described along with their basic units. Examples are provided to illustrate stating measurements with the correct unit.
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The document discusses units of measurement used in chemistry. It introduces common units like meters, liters, grams, seconds that are used to measure length, volume, mass and time. These units make up the International System of Units (SI) and metric system which are decimal systems used widely in science. Examples are given of measuring tools and conversions between units like inches to centimeters. Key types of measurements covered are length, volume, mass, temperature and time.
Units of measurement
This document discusses units of measurement and measurement tools. It covers common units used to measure length, volume, weight, and temperature in both U.S. customary and metric systems. Key tools for measurement include thermometers, measuring cups, graduated cylinders, watches, and scales. The document also emphasizes that every measurement includes a number and corresponding unit from the measuring device or system used.
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The document discusses units of measurement used in the metric system for length, mass, volume, and time. It explains that the metric system uses SI units which are based on meters, kilograms, seconds, and kelvins. It differentiates between mass, which is a measure of the amount of matter, and weight, which is the force exerted by mass due to gravity. Various tools for measurement are also introduced, such as balances, scales, graduated cylinders and thermometers.
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Learning Objectives
Define the International System of Units (measurement system).
Define a unit of measurement and demonstrate the ability to convert measurements.
Define length, temperature, time, volume, mass, density, and concentration.
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Just like you and your friend communicate using the same language, scientists all over the world need to use the same language when reporting the measurements they make. This language is called the metric system. In this lesson we will cover the metric units for length, mass, density, volume and temperature, and also discuss how to convert among them.
Metric Measurement
What do all of these words have in common: thermometer, barometer, diameter, odometer and parameter? All of these words end in
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measure
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The units of measure in the English and metric systems
Most Americans are taught the English or standard system of measurement, but never get a good dose of the metric system. Lucky for you, it is a much easier system to learn than the English system because all the measurements are
base 10
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10
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Because you may not be used to thinking metrically, it may take a little practice using and working with the metric system before you gain a better understanding of it and become more fluent in the measurement language of scientists (and most non-Americans). I challenge you to sprinkle a little more metric in your life. Maybe read the milliliter measurement on your soda can or glance at the kilometer reading on your speedometer. Being able to picture metric quantities will really help with the rest of this course.
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1
Exercise 1
THE CALORIE
INTRODUCTION
All animals, including humans, need to consume energy in order to survive. We
call this energy food. The unit which is used to describe the energy content of food is
the Calorie (food calorie, note the capital ‘C’). One calorie (note the lower case ‘c’) is the
energy required to raise one gram of water by one degree Celsius. The food Calorie is
defined as 1000 calories or one kilocalorie (kcal). Most scientists not dealing with food
now use other units such as joules or British Thermal Units (BTUs) to measure energy,
but the Calorie is still used to describe food energy.
The Calories in food are measured using a CALORIMETER, which is a special
combustion device designed to burn food samples completely and capture the energy in
a water jacket. For a 100% efficient calorimeter, the energy captured is equal to the
energy content of the food as shown below:
Energy captured = (mass of water) ´ c ´ (Temp. change) = Energy Content (1)
The constant c is the specific heat of water and is equal to 1
Cg
cal
°
(one calorie per
gram per degree C). In our case, however, the calorimeter we use will capture only a
fraction of the total energy, so we must account for this reduced efficiency.
THE CALORIMETER
The device that scientists use to capture the heat energy of a combustible mixture
is a bomb calorimeter. It is a metal chamber which is supplied with a measured amount
of oxygen during the combustion of the test material. The heat from the burning
material is transferred to a water reservoir that surrounds the metal chamber containing
the test material. The change in temperature is used to determine the number of calories
that the material originally held. A bomb calorimeter is very nearly 100% efficient. It is
also very dangerous (thus the name ‘bomb’ calorimeter) and so we will use a simpler
(but less efficient) type of calorimeter.
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The simple but effective calorimeter we will use consists of a calorimeter can (a
metal cylinder with a notch out of the bottom), a calorimeter lid to hold a 125 ml flask, a
flask stopper and thermometer, a sample holder and some tools. Each group of students
will have their own calorimeter to use. Because these simple calorimeters are not 100%
efficient, the water will not capture all of the energy content of the food. Therefore, the
equation for this calorimeter must be modified to:
Energy captured = (mass of water) ´ c ´ (Temp. change) = Energy Content ´ e (2)
where e is the efficiency of energy capture by the water. With this equation and a food
item of known caloric content, we can determine the efficiency of our calorimeter and
2
explore why the efficiency might vary from one group to another. Once a consistent
efficiency is achieved, we can use that efficiency to determine the caloric content of any
combustible item.
OBJECTIVES:
1) To measure the energy content of a food sample. ...
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The document discusses measurement and units of measurement. It begins by defining measurement and explaining its importance. It then distinguishes between standard and non-standard units, and describes the English and metric systems of measurement. The key types of measurement covered are length, mass, volume/capacity, and temperature. Basic metric units for each type are provided. The document concludes with an activity asking students to identify measurement units.
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This document provides an overview of scientific measurement and units covered in a general chemistry course. It discusses the metric system of units used in science including the SI base units. It also covers scientific notation, significant figures, units of temperature, density, specific gravity, and heat measurement.
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This document covers several topics related to measurement and error analysis in physics experiments. It begins by defining accuracy and precision, distinguishing between the two concepts. Accuracy refers to how close a measurement is to the true value, while precision describes the degree of variation in repeated measurements of the same quantity. It then discusses random and systematic errors, explaining that random errors vary unpredictably while systematic errors remain constant. The document provides examples of different types of systematic errors like instrumental, environmental, and observational errors. Finally, it introduces concepts like absolute error, relative error, and percentage error to quantify the uncertainty in measurements.
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The document provides information about metric units of length, mass, and volume. It compares metric and English units and provides conversions between units. For length, it states that the meter is the base SI unit and provides conversions such as 1 kilometer = 1000 meters. For mass, it indicates the gram is the base unit and gives conversions like 1 kilogram = 1000 grams. For volume, it notes the liter is the base unit and provides the conversion 1 liter = 1000 milliliters.
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This document describes procedures for measuring various properties including size distribution, mass distribution, concentration, temperature, and volume. The procedures involve carefully measuring samples and recording the measurements and observations. Key steps include choosing a representative sample, using proper measuring tools, accounting for errors and uncertainties, and recording all relevant data. The goal is to obtain large data sets that can be statistically analyzed to evaluate results and understand sources of error.
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Chapter 3 scientific measurement 1
The document outlines objectives and concepts related to scientific measurement in chemistry, including defining units in the International System of Units (SI) such as meters, kilograms, and kelvins; distinguishing between accuracy and precision in measurements; and explaining the proper handling of significant figures in measurements and calculations.
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