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# Chapter Two - PowerPoint PPT Presentation

Fundamentals of General, Organic, and Biological Chemistry 5th Edition. Chapter Two. Measurements in Chemistry. James E. Mayhugh Oklahoma City University  2007 Prentice Hall, Inc. Outline. 2.1 Physical Quantities, Metric System 2.2 Measuring Mass

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5th Edition

### Chapter Two

Measurements in

Chemistry

James E. Mayhugh

Oklahoma City University

2007 Prentice Hall, Inc.

• 2.1 Physical Quantities, Metric System

• 2.2 Measuring Mass

• 2.3 Measuring Length and Volume

• 2.4 Measurement and Significant Figures

• 2.5 Scientific Notation

• 2.6 Rounding Off Numbers

• 2.7 Converting a Quantity from One Unit to Another

• 2.8 Problem Solving: Estimating Answers

• 2.9 Measuring Temperature

• 2.10 Energy and Heat

• 2.11 Density

• 2.12 Specific Gravity

Chapter Two

Physical properties such as height, volume, and temperature that can be measured are called physical quantities. Both a number and a unit of defined size is required to describe physical quantity.

Chapter Two

Chapter Two

• Scientists work with both very large and very small numbers.

• Prefixes are applied to units to make saying and writing measurements much easier.

• The prefix pico (p) means “a trillionth of.”

• The radius of a lithium atom is 0.000000000152 meter (m). Try to say it.

• The radius of a lithium atom is 152 picometers (pm). Try to say it.

Chapter Two

Chapter Two

• Mass is a measure of the amount of matter in an object. Mass does not depend on location.

• Weight is a measure of the gravitational force acting on an object. Weight depends on location.

• A scale responds to weight.

• At the same location, two objects with identical masses have identical weights.

• The mass of an object can be determined by comparing the weight of the object to the weight of a reference standard of known mass.

Chapter Two

a) The single-pan balance with sliding counterweights. (b) A modern electronic balance.

Chapter Two

Relationships between metric units of mass and the mass units commonly used in the United States are shown below.

Chapter Two

Problem units commonly used in the United States are shown below.

Express 3.27 mg in units of grams.

Express 19.3 kg in units of mg.

Chapter Two

2.3 Measuring Length and Volume units commonly used in the United States are shown below.

• The meter (m) is the standard measure of length or distance in both the SI and the metric system.

• Volume is the amount of space occupied by an object. A volume can be described as a length3.

• The SI unit for volume is the cubic meter (m3).

Chapter Two

Relationships between metric units of length and volume and the length and volume units commonly used in the United States are shown below and on the next slide.

Chapter Two

A m the length and volume units commonly used in the United States are shown below and on the next slide.3 is the volume of a cube 1 m or 10 dm on edge. Each m3 contains (10 dm)3 = 1000 dm3 or liters. Each liter or dm3 = (10cm)3 =1000 cm3 or milliliters. Thus, there are 1000 mL in a liter and 1000 L in a m3.

Chapter Two

The metric system is based on factors of 10 and is much easier to use than common U.S. units. Does anyone know how many teaspoons are in a gallon?

Chapter Two

2.4 Measurement and Significant Figures easier to use than common U.S. units. Does anyone know how many teaspoons are in a gallon?

• Every experimental measurement has a degree of uncertainty.

• The volume, V, at right is certain in the 10’s place, 10mL<V<20mL

• The 1’s digit is also certain, 17mL<V<18mL

• A best guess is needed for the tenths place.

Chapter Two

• To indicate the precision of a measurement, the value recorded should use all the digits known with certainty, plus one additional estimated digit that usually is considered uncertain by plus or minus 1.

• No further insignificant digits should be recorded.

• The total number of digits used to express such a measurement is called the number of significant figures.

• All but one of the significant figures are known with certainty. The last significant figure is only the best possible estimate.

Chapter Two

Below are two measurements of the mass of the same object. The same quantity is being described at two different levels of precision or certainty.

Chapter Two

• When reading a measured value, all nonzero digits should be counted as significant. There is a set of rules for determining if a zero in a measurement is significant or not.

• RULE 1. Zeros in the middle of a number are like any other digit; they are always significant. Thus, 94.072 g has five significant figures.

• RULE 2. Zeros at the beginning of a number are not significant; they act only to locate the decimal point. Thus, 0.0834 cm has three significant figures, and 0.029 07 mL has four.

Chapter Two

• RULE 3. counted as significant. There is a set of rules for determining if a zero in a measurement is significant or not.Zeros at the end of a number and after the decimal point are significant. It is assumed that these zeros would not be shown unless they were significant. 138.200 m has six significant figures. If the value were known to only four significant figures, we would write 138.2 m.

• RULE 4. Zeros at the end of a number and before an implied decimal point may or may not be significant. We cannot tell whether they are part of the measurement or whether they act only to locate the unwritten but implied decimal point.

Chapter Two

2.5 Scientific Notation counted as significant. There is a set of rules for determining if a zero in a measurement is significant or not.

• Scientific notation is a convenient way to write a very small or a very large number.

• Numbers are written as a product of a number between 1 and 10, times the number 10 raised to power.

• 215 is written in scientific notation as:

215 = 2.15 x 100 = 2.15 x (10 x 10) = 2.15 x 102

Chapter Two

Two examples of converting scientific notation back to standard notation are shown below.

Chapter Two

• The distance from the Earth to the Sun is 150,000,000 km. Written in standard notation this number could have anywhere from 2 to 9 significant figures.

• Scientific notation can indicate how many digits are significant. Writing 150,000,000 as 1.5 x 108 indicates 2 and writing it as 1.500 x 108 indicates 4.

Chapter Two

2.6 Rounding Off Numbers Written in standard notation this number could have anywhere from 2 to 9 significant figures.

• Often when doing arithmetic on a pocket calculator, the answer is displayed with more significant figures than are really justified.

• How do you decide how many digits to keep?

• Simple rules exist to tell you how.

Chapter Two

RULE 1. Written in standard notation this number could have anywhere from 2 to 9 significant figures.In carrying out a multiplication or division, the answer cannot have more significant figures than either of the original numbers.

Chapter Two

• RULE 2. Written in standard notation this number could have anywhere from 2 to 9 significant figures.In carrying out an addition or subtraction, the answer cannot have more digits after the decimal point than either of the original numbers.

Chapter Two

Rounding Written in standard notation this number could have anywhere from 2 to 9 significant figures.

• RULE 1. If the first digit you remove is 4 or less, drop it and all following digits.

2.4271 becomes 2.4 when rounded off to two significant figures.

• RULE 2. If the first digit removed is 5 or greater, round up by adding 1 to the last digit kept.

4.5832 is 4.6 when rounded off to 2 significant figures.

• If a calculation has several steps, it is best to round off at the end.

Chapter Two

Problems Written in standard notation this number could have anywhere from 2 to 9 significant figures.

Express 1,066,298 to 5 significant figures using scientific notation.

Express 2/3 to 4 significant figures.

Chapter Two

Problem Written in standard notation this number could have anywhere from 2 to 9 significant figures.

Determine the answer to:

6.023 x 1023 x 2.32 x 10-7

______________________________

Calculator gives too many significant figures

14.4536 x 1016 ??

1.45 x 1017(3 sig. figures)

Chapter Two

• Factor-Label Method: A quantity in one unit is converted to an equivalent quantity in a different unit by using a conversion factor that expresses the relationship between units.

(Starting quantity) x (Conversion factor) = Equivalent quantity

Chapter Two

Writing 1 km = 0.6214 mi as a fraction restates it in the form of a conversion factor. This and all other conversion factors are numerically equal to 1.

The numerator is equal to the denominator. Multiplying by a conversion factor is equivalent to multiplying by 1 and so causes no change in value.

Chapter Two

When solving a problem, the idea is to set up an form of a conversion factor. This and all other conversion factors are numerically equal to 1.

equation so that all unwanted units cancel, leaving only the desired units.

Chapter Two

Problem form of a conversion factor. This and all other conversion factors are numerically equal to 1.

An infant weighs 9.2 lb at birth. How many kg does the infant weigh?

1kg = 2.205 lb is the conversion factor

Chapter Two

Problem form of a conversion factor. This and all other conversion factors are numerically equal to 1.

The directions on the bottle of cough syrup say to give 4.0 fl oz to the child, but your measuring spoon is in units of mL. How many mL should you administer?

1 L = 0.264 gal

1 gal = 4 qt

1 qt = 32 fl oz

1L = 1000 mL

Chapter Two

Problem 2.15 form of a conversion factor. This and all other conversion factors are numerically equal to 1.from McMurry:

One international nautical mile is defined as exactly 6076.1155 ft, and a speed of 1 knot is defined as one nautical mile per hour. What is the speed in m/sec of a boat traveling at 14.3 knots?

What we know:

1 knot = 1 naut. mi/hr = 6076.1155 ft/hour

1 ft = 0.3048 m

1 hr = 60 min

1 min = 60 sec

Chapter Two

Problem Solved ! form of a conversion factor. This and all other conversion factors are numerically equal to 1.

Chapter Two

2.9 Measuring Temperature form of a conversion factor. This and all other conversion factors are numerically equal to 1.

• Temperature is commonly reported either in degrees Fahrenheit (oF) or degrees Celsius (oC).

• The SI unit of temperature is the Kelvin (K).

• 1 Kelvin, no degree, is the same size as 1 oC.

• 0 K is the lowest possible temperature, 0 oC = 273.15 K is the normal freezing point of water. To convert, adjust for the zero offset.

• Temperature in K = Temperature in oC + 273.15

• Temperature in oC = Temperature in K - 273.15

Chapter Two

Freezing point of H form of a conversion factor. This and all other conversion factors are numerically equal to 1.2O Boiling point of H2O

32oF 212oF

0oC 100oC

212oF - 32oF = 180oF covers the same range of temperature as 100oC - 0oC = 100oC covers. Therefore, a Celsius degree is exactly 180/100 = 1.8 times as large as a Fahrenheit degree. The zeros on the two scales are separated by 32oF.

Chapter Two

Fahrenheit, Celsius, and Kelvin temperature scales. form of a conversion factor. This and all other conversion factors are numerically equal to 1.

Chapter Two

Chapter Two

Problem to converting between different units of length or volume, but is a little more complex. The different size of the degree

Problem

A patient has a temperature of 38.8oC. What is her temperature in oF?

We know 2 equations:

oF = (1.8 x oC) + 32

oC = (oF – 32)/1.8

Chapter Two

2.10 Energy and Heat to converting between different units of length or volume, but is a little more complex. The different size of the degree

• Energy: The capacity to do work or supply heat.

• Energy is measured in SI units by the Joule (J); the calorie is another unit often used to measure energy.

• One calorie (cal) is the amount of heat necessary to raise the temperature of 1 g of water by 1°C.

• A kilocalorie(kcal) = 1000 cal. A Calorie, with a capital C, usedby nutritionists, equals 1000 cal.

• An important energy conversion factor is:

1 cal = 4.184 J

Chapter Two

• Not all substances have their temperatures raised to the same extent when equal amounts of heat energy are added.

• One calorie raises the temperature of 1 g of water by 1°C but raises the temperature of 1 g of iron by 10°C.

• The amount of heat needed to raise the temperature of 1 g of a substance by 1°C is called the specific heat of the substance.

• Specific heat is measured in units of cal/gC

Chapter Two

• Knowing the same extent when equal amounts of heat energy are added.mass and specific heat of a substance makes it possible to calculate how much heat must be added or removed to accomplish a given temperature change.

• (Heat Change) = (Mass) x (Specific Heat) x (Temperature Change)

• H in cal; mass in g; C in cal/goC; Temp in oC

• Using the symbols D for change, H for heat, m for mass, C for specific heat, and T for temperature, a more compact form is:

DH = mCDT

Chapter Two

Problem same extent when equal amounts of heat energy are added.

What is the specific heat of Aluminum if it takes 161 cal to raise the temperature of 75 g of Al by 10.0oC?

DH = mCDT

solve for C (specific heat, cal/g.oC)

Chapter Two

2.11 same extent when equal amounts of heat energy are added.Density

Density relates the mass of an object to its volume. Density is usually expressed in units of grams per cubic centimeter (g/cm3) for solids, and grams per milliliter (g/mL) for liquids.

Mass (g)

Density =

Volume (mL or cm3)

Chapter Two

Problem same extent when equal amounts of heat energy are added.

What volume in mL should you measure out if you need 16 g of ethanol which has a density of 0.79 g/mL? (You only have a graduated cylinder, no balance.)

Chapter Two

Chapter Two

2. 12 Specific Gravity same extent when equal amounts of heat energy are added.

Specific gravity(sp gr):density of a substance divided by the density of water at the same temperature. Specific gravity is unitless. The density of water is so close to 1 g/mL that the specific gravity of a substance at normal temperature is numerically equal to the density.

Density of substance (g/ml)

Specific gravity =

Density of water at the same temperature (g/ml)

Chapter Two

The specific gravity of a liquid can be measured using an instrument called a hydrometer, which consists of a weighted bulb on the end of a calibrated glass tube. The depth to which the hydrometer sinks when placed in a fluid indicates the fluid’s specific gravity.

Chapter Two

Chapter Summary instrument called a hydrometer, which consists of a weighted bulb on the end of a calibrated glass tube. The depth to which the hydrometer sinks when placed in a fluid indicates the fluid’s specific gravity.

• Physical quantitiesrequire a number and a unit.

• Preferred units are either SI units or metric units.

• Mass, the amount of matter an object contains, is measured in kilograms(kg) or grams(g).

• Length is measured in meters(m). Volume is measured in cubic metersin the SI system and in liters(L) or milliliters(mL) in the metric system.

• Temperature is measured in Kelvin(K) in the SI system and in degrees Celsius(°C) in the metric system.

Chapter Two

Chapter Summary Cont. instrument called a hydrometer, which consists of a weighted bulb on the end of a calibrated glass tube. The depth to which the hydrometer sinks when placed in a fluid indicates the fluid’s specific gravity.

• The exactness of a measurement is indicated by using the correct number of significant figures.

• Significant figures in a number are all known with certainty except for the final estimated digit.

• Small and large quantities are usually written in scientific notationas the product of a number between 1 and 10, times a power of 10.

• A measurement in one unit can be converted to another unit by multiplying by a conversion factorthat expresses the exact relationship between the units.

Chapter Two

Chapter Summary Cont. instrument called a hydrometer, which consists of a weighted bulb on the end of a calibrated glass tube. The depth to which the hydrometer sinks when placed in a fluid indicates the fluid’s specific gravity.

• Problems are solved by the factor-label method.

• Units can be multiplied and divided like numbers.

• Temperature measures how hot or cold an object is.

• Specific heat is the amount of heat necessary to raise the temperature of 1 g of a substance by 1°C.

• Density relates mass to volume in units of g/mL for a liquid or g/cm3 for a solid.

• Specific gravity is density of a substance divided by the density of water at the same temperature.

Chapter Two