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Scientific Notation Scientific Notation is a method of writing numbers so that only significant digits are shown. e.g. the distance from the earth to the moon is reported as: in common notation: 382 000 km in scientific notation: 3.82 105 km In scientific notation a number has one nonzero digit to the left of the decimal point and is multiplied by the appropriate power of 10 (either positive or negative). Scientific notation is especially useful in concisely reporting very large or very small numbers. e.g. the number of electrons in a coulomb of charge is: in common notation: 6 242 000 000 000 000 000 in scientific notation: 6.242 1018 Web Users please note: the mass of a proton is : in common notation: 0.000 000 000 000 000 000 000 000 001 672 kg in scientific notation: 1.672 10-27 kg the number of particles in a mole of substance is: in common notation: 602 200 000 000 000 000 000 000 in scientific notation: 6.022 1023 Answers to these questions are on page 23 & 24, i.e., at the end of this unit. Practice: 1. Express the following in scientific notation. a) b) c) 68090 0.000 023 5400 ________________________ ________________________ ________________________ d) 0.80 ________________________ e) 0.050 40 ________________________ 2. Express the following in common notation. a) 7 101 _______________________ b) 4.098 10-3 _______________________ c) 8.3 107 _______________________ d) 10.1 10-5 ____________________________ Units & Errors 1 SIGNIFICANT FIGURES (Sig Figs) = all digits known for sure plus 1 more digit 1. During the manufacture of steel from iron ore, the ore is fed into a large kiln whose temperature increases from less than 400 C at the top to about 1600 C at the bottom. The thermometer shown below indicates various kiln temperatures A through E. For each of these, record the temperature in common notation, the number of significant digits, and the temperature in scientific notation. 1000 C 800 1200 B D 600 1400 E A 400 1600 ºC KILN TEMPERATURE common notation number of sig figs scientific notation A B C D E Using a thermometer which is more finely calibrated gives readings with more sig figs. Repeat the previous exercise for temperatures A and C using the thermometer shown below. 1000 C 800 1200 B D 600 1400 E A 400 1600 ºC KILN TEMPERATURE common notation number of sig figs scientific notation A C Units & Errors 2 SIG FIGS (continued) 2 a) An automobile tachometer measures engine speed in revolutions per minute (rpm). In the tachometer shown, engine speeds to the nearest 100 rpm are displayed, i.e., two tailing zeros are present in all readings- they never change. In case A, below, an automobile is idling at rest and, in case B, the automobile is moving at a steady speed of 90 km/h. For both cases, report the rpm reading in common notation, the number of significant digits, and the rpm reading in scientific notation. Digital instruments do not allow the observer to estimate a final digit. Assume that the first digit to the left of the zeros is a number which is estimated by the instrument. 700 rpm 2300 rpm A B common notation number of sig figs scientific notation A B b) Repeat the previous exercise assuming that the tachometer reads to the nearest 10 rpm's. common notation number of sig figs scientific notation A B c) Repeat the previous exercise assuming that the tachometer reads to the nearest 1 rpm. common notation number of sig figs scientific notation A B Units & Errors 3 Sig Figs (continued) 3. The length of a desk top is measured with 3 different meter sticks (A, B, and C) as shown below. For each meter stick, record the length of the desk top in common notation, the number of sig figs, and the length in scientific notation. 0 A 1 0 .1 .2 .3 .4 .5 .6 .7 .8 .9 1.0 .1 .2 0 .1 .2 .3 .4 .5 .6 .7 .8 .9 1.0 .1 .2 common notation number of sig figs B C scientific notation A B C How does the sensitivity of a measuring instrument affect the number of significant figures obtainable in a measurement? Note that by using ruler A we are able to exactly measure the object's length to the nearest meter and estimate the length to the nearest 0.1 meters (2 sig figs). Note that by using ruler B we are able to exactly measure the object's length in meters and in 0.1 meters and estimate the length to the nearest 0.01 meters (3 sig figs). Note that by using ruler C we are able to exactly measure the object's length in meters, 0.1 meters, and 0.01 meters and estimate the length to the nearest 0.001 meters (4 sig figs). In general, the smallest unit we can exactly measure is the smallest division of our measuring instrument. We may then estimate 1 digit more. All of these (and only these) digits are significant digits (sig figs). Units & Errors 4 Sig Figs (continued) 4. For each of the automobile gages shown below, record the gage reading in common notation, the number of sig figs, and the length in scientific notation. 180 170 190 200 160 ENGINE TEMPERATURE 150 210 ºF 70 60 50 80 90 40 100 30 110 20 10 120 SPEED km / h common notation 130 number of sig figs scientific notation engine temp. (ºF) speed (km/h) Units & Errors 5 Rules for Significant Digits in Numbers 1. Nonzero digits: 1, 2, 3, 4, 5, 6, 7, 8, and 9 are always significant. 6.2 16.2 16.25 two significant digits three significant digits four significant digits 2. Leading zeros: zeros that appear at the start of a number, are never significant because they act only to fix the position of the decimal point in a number less than 1. ` 0.564 0.0564 three significant digits three significant digits 3. Confined zeros: that appear between nonzero numbers are always significant. 104 1004 three significant digits four significant digits 4. Trailing zeros: zeros at the end of a number are significant only if: a) the number contains a decimal point or b) the number contains an overbar 15400 three significant digits 1540.0 five significant digits 15.4000 six significant digits 5,600 four significant digits or 5.600 103 5,600 three significant digits or 5.60 103 Practice: Determine the number of significant digits in the following numbers: a) 345 _______ i) b) 32000 c) 0.0078 _______ d) 9.0068 _______ e) 5.0200 _______ g) h) 10700 122.0 10.04 Units & Errors _______ _______ j) f) 20 0.604 _______ _______ _______ _______ 6 Uncertainty in Measurement In scientific work, we recognize two kinds of numbers: exact numbers - values known exactly - numbers which are defined or counted - defined: 12 donuts in a dozen 1000 grams in a kilogram -counted: 25 students in a classroom inexact numbers - values are uncertain - numbers which are measured eg. - speed of an automobile - temperature of a cup of soup - volume of water in a beaker Exact numbers are assigned an infinite number of significant figures for calculations Inexact numbers have a number of significant figures equal to the number of digits known for certain plus one more. Significant Figures in Calculations One additional digit (one more than the number of sig figs) is usually carried on all values throughout a calculation and the answer is rounded to the correct number of sig figs. In calculations involving multiplication, division, roots, and powers: round off the answer so that it has only as many significant figures as the value in the calculation with the fewest significant digits. e.g. 35.63 0.5481 0.0530 100% 88.5470578% 88.5% 1.1689 The answer only contains 3 significant figures since this is the least number of sig figs amoung the values in the calculation. 100 % is an exact number having an infinite number of significant digits. In addition and subtraction: the answer is only as precise as the least precise measurement. The answer has as many decimal places as the value with the least. e.g. Suppose we have 3 measurements of length to be added, i.e., 6.6 m 18.74 m 0.766 m 26.106 m 26.1 m Note that the least precise measurement, 6.6 m, was only reported to the nearest 0.1m, therefore the answer cannot be reported with greater precision. Note that the correct answer has more significant digits than one of the measurements. Remember that the answer of additions or subtractions cannot have more precision than the least precise measurement. For example, if approx. 1 L of Pepsi is divided equally between 3 people, each person will not get 0.333 L, but rather 0.3L. Units & Errors 7 Accuracy and Precision Accuracy refers to how closely a measured value agrees with the correct value. Precision refers to how closely individual measurements agree with each other. A group of measurements may be very precise (agree closely) but still be inaccurate. Ideally, all measurements should be both precise and accurate. precise but not accurate accurate and precise not accurate or precise Rounding off Numbers If the digit following the last significant digit is greater than 5, the number is rounded up to the next higher digit: 9.47 to 2 significant digits = 9.5 If the digit following the last significant digit is less than 5, the number is rounded to the present value of the last significant digit: 9.43 to 2 significant digits = 9.4 If the last digit is exactly 5, the number is rounded to the nearest even digit: 8.65 to 2 significant digits = 8.6 8.75 to 2 significant digits = 8.8 8.55 to 2 significant digits = 8.6 Practice: Round the following numbers to 2 sig figs. a) 2249 _____ d) b) 2250 _____ e) 0.07750 ____ c) 2251 _____ f) 0.07749 ____ Units & Errors 2250.001 ____ 8 SI Base Units Quantity Name of unit Symbol for unit length metre m mass kilogram kg time second s amount of substance mole mol temperature kelvin K electric current ampere A luminous intensity candela cd Conversion Factors Unit Equivalent 1 inch (in) 2.54 cm 1 foot (ft) 12 in 1 yard (yd) 0.9 144 m 1 metre (m) 39.37 in = 3.28084 ft 1 mile 1 760 yd = 1.609 km 1 pound (lb) 453.6 g 1 kilogram (kg) 2.205 lb 1 grain (gr) 64.8 mg 1 ton (ton) - short 2 000 lb = 907 kg 1 ton (ton) - long 2 240 lb 1 tonne (t) - metric 2 205 lb = 1000 kg 1 imperial gallon (gal) 4.546 L 1 U.S. gallon (gal) 3.785 L 1 imperial fluid ounze (fl oz) 28.41 mL or cc 1 U.S. fluid ounze (fl oz) 29.57 mL or cc 1 imperial quart (qt) 1.136 L 1 U.S. quart (qt) 0.946 L Memorize: Units & Errors 1mL = 1cm3 = 1cc 1 L = 1000 mL = 1000 cm3 = 1000 cc = 1 dm3 1000 L = 1m3 9 Decimal Multipliers Prefix Symbol Mult. Factor e.g. meters e.g. meters exa E 1018 1 Em = 1018 m 10-18 Em = 1 m peta P 1015 1 Pm =1015 m 10-15 Pm = 1 m tera T 1012 1 Tm = 1012 m 10-12 Tm = 1 m giga G 109 1 Gm =109 m 10-9 Gm = 1 m mega M 106 1 Mm = 106 m 10-6 Mm = 1 m kilo k 103 1 km = 103 m 10-3 km = 1 m hecto h 102 1 hm = 102 m 10-2 hm = 1 m deca da 10 1 dam = 10 m 10-1 dam = 1 m 1 1m=1m 1m=1m base unit deci d 10-1 1 dm = 10-1 m 10 dm = 1 m centi c 10-2 1 cm = 10-2 m 102 cm =1 m milli m 10-3 1 mm = 10-3 m 103 mm = 1 m micro 10-6 1 m = 10-6 m 106 m = 1 m nano 10-9 1 m = 10-9 m 109 m = 1 m pico 10-12 1 m = 10-12 m 1012 m = 1 m femto f 10-15 1 fm = 10-15 m 1015 fm = 1 m atto a 10-18 1 am = 10-18 m 1018 am = 1 m Units & Errors 10 DECIMAL MULTIPLIERS APPLIED TO UNITS 1 Ms = s 1s= Ms 1 kg = g 1g= kg 1 dL = L 1L= dL 1 cm = m 1m= cm 1 mol = mol 1 mol.= 1 m = m 1m= m 1 mg = g 1s= Gs 1 g = g 1m= mm Units & Errors mol. 11 Converting Units Using the ‘Unit Factor’ Method (‘Dimensional Analysis’) Multiply the given unit by conversion factors. We will start with a simple example and then progress to more difficult examples. Learn the procedure by working through the examples. Example 1: Convert 3 minutes to seconds. CONVERSION FACTORS Step 1: Write down the problem as shown below and decide what conversion factors you will need. ? s = 3 min 60 s = 1 min Step 2: Get the conversion factors. Include units. Step 3: Set up the calculation using the units. Then cancel the units (as if they were numbers) to ensure that the conversion factors are set up correctly. ? s 3 min s min s If the factor is upside down, the units of the answer make no sense. Check this. Do not leave out the units as the units will help you avoid errors. For example: This unit makes no sense so min ? s 3 min s min 2 . s the conversion factor must be upside-down. Step 4: Put the numbers in the conversion factors and calculate the correct answer. 60 s ? s 3 min 1 min 180 s Steps 3 and 4 can be done simultaneously but do not leave out the units. They are the key to success. Plan your conversions using arrows. There will be one conversion factor for each arrow. Example 2: Convert 4 days to seconds. 3 Step1: ?s 2 min 1 h = 2 1 Step 4: 2 1 h = 60 min 3 h min s ? s 4 da da h min Step 3: Step 2: 1 min = 60 s 4 da 1 1 da = 24 h s 3 24 h 60 min 60 s ? s 4da 345,600 s 1 da 1 h 1 min Units & Errors 12 Example 3: Convert 37 mi/h to m/s 2 Step 1: km ? m/s = 1 mi/h Step 2: 3 Step 3 and 4: 2 1 1 mi = 1.609 km 1 km = 103 m 1 h = 3600 s 3 m mi 1.609 km 10 m 1 h m ? 37 16.5 s h 1 mi 1 km 3600 s s 3 Example 4: Gold has a mass density of 19.30 g/cm3. Convert this to units of kg/m3. 1 ? kg/m3 Step 1: Step 2: 19.30 g/cm3 = 1 kg = 103 g (1 m = 102 cm)3 1 m3 = 106 cm3 2 Step 3 and 4: 1 2 kg g 1 kg 10 6 cm3 kg 19300 3 ? 3 19.30 m cm3 103 g 1 m3 m The Metric Multipliers Technology students are expected to memorize the metric multipliers shown below. Use them to solve the conversion problems on the following page. giga mega kilo G M k 109 106 103 Units & Errors base unit deci centi milli d 1 c m 10-1 10-2 10-3 micro nano pico p 10-6 10-9 10-12 13 Convert and express in correct scientific notation. _______ 1. 2.0 1010 L dL _______ 2. 5.08 106 in km _______ 3. 5.91 10-3 ks cs _______ 4. 3.0 10-2 m3 mL _______ 5. 9.00 102 g lb _______ 6. 4.56 10-4 Ms ms _______ 7. 0.000 002 km fm _______ 8. 101 g g _______ 9. 25 dm mm _______ 10. 8.42 mmol kmol _______ 11. 5.0 105 mol mol _______ 12. 7.10 103 kgm-3 g / L Units & Errors 14 Unit Conversion Problems 1. Convert 142 Ms to leap years. ( 366 da = 1 lp. yr ) 2. A window sized air conditioner rated at 8000 B.T.U. will remove 8000 B.T.U. of heat in one hour. How many calories of heat is this? 1 B.T.U. = 1.0541010 ergs 1 erg = 10-7 joules 4.184 joules = 1 cal. 3. The driver of a Honda Civic claims he gets 50 miles per gallon (mpg). Convert this to litres per 100 km. 1 mile = 1.609 km. 4.546 L. = 1 Imp. gallon 4. The density of pure gold is 19.32 g / mL. Calculate its density in units of kg / m3. Units & Errors 15 Problem Solving By Logical Statements: Relying on the method of Ratio and Proportion to solve technology problems will often prove uncessful. No chemistry text book written within the last 20 years has taught ratio and proportion as a method for converting units. With minimal investment of time (practice), you will be convinced that the unit factor method (just presented) is much quicker and more effective than ratio and proportion for converting units. Also, for general problem solving in technology, ratio and proportion is inadequate and will often lead to incorrect answers. An adaptation of ratio and proportion, called ‘solving by logical statements’ is easy to use and will improve your exam scores because you will correctly solve more problems using it. Logical statements are especially well suited for dilution and concentration calculations in chemistry. We will apply the method of logical statements, first, to a simple problem. The same pattern is then applied to all other problems. The Method of Logical Statements: Problem: 12 eggs cost 60¢. How much do 6 eggs cost? Solution: You will intuitively know that 6 eggs cost ½ as much as 12 eggs so you will divided 60¢ by 2 and get 30¢. This is, of course, correct, but why did you divide by 2? Because, in your head you calculated: 6 eggs 1/2 12 eggs or 12 eggs 2 6 eggs You determined a ratio or ‘factor’ of the two known values, then multiplied or divided by that factor 60¢ ½ i.e., or 60¢ 2 Don’t you wish all chemistry problems were that simple? The truth is that most are if use this same simple, logical method to solve your problems. Let’s write out this method in a standard format. 12 eggs cost 60¢ 6 eggs 1 = 60¢ = 30¢. 6 eggs cost x¢ = 60¢ 2 12 eggs 1. Write 2 statement lines, one immediately below the other, inserting ‘x’ for the value to be solved for. At this point it looks like the set up for ratio and proportion, but do not cross multiply. 2. Bring down the known value (60¢) with its unit. See the arrow. Do not leave out the unit. The known value that has the same unit as the answer will have. 3. Multiply the known value (60¢) by a ratio (or factor) of the two egg values. You only have 6 eggs 12 eggs or . Choose the one that makes sense, i.e., two choices, either 12 eggs 6 eggs fewer eggs should cost less. Include the units but note that the units of eggs will cancel leaving the correct unit (¢). Units & Errors 16 There are two reasons why you will successfully solve more problems by this method than by ratio and proportion: a) The units are carried. Some will cancel leaving the correct unit for the answer. In ratio and proportion, units are never carried because when they are cross multiplied they make no sense. In the example above, the unit obtained by cross multiplying is ‘eggs¢’, which has no meaning. b) You make a logical decision in setting up the ratio, i.e., you multiply by ½ not by 2, because fewer eggs must cost less money. Ratio and proportion is a mechanical, mindless operation, i.e., simply cross multiplying. In many technology problems this will be incorrect as we will illustrate in the following examples. Example 2: A Honda Civic with a 1.3 L engine gets 50 miles per gallon (mpg). Calculate the gas mileage (mpg) of a 5.0 L Ford Mustang assuming gas mileage depends only upon engine size. Solution: Honda: 1.3 L engine gets 50 mpg 1.3 L Mustang: 5.0 L engine gets x mpg = 50 mpg = 13 mpg 5.0 L The ratio (1.3/5.0) is chosen because it makes sense that a larger engine gets lower gas mileage. Crossmultiplying, as one might do using ratio and proportion, yields a ridiculous answer (192 mpg)! This problem is an example of an inverse relationship. Inverse relationships are common in technology, e.g., pressure-volume, mass-velocity, volume-concentration, age-beauty. For such problems one parameter is increasing while the other is decreasing. The egg problem was an example of a direct relationship. Direct relationships are those in which both parameters increase or decrease simultaneously. Cross multiplying and the unit factor method work for direct relationships but not for indirect relationships. When converting a distance of 1 km to meters, the relationship can be thought of as direct even though the distance is not changing. But note that the greater the value in km, the greater will be the value in meters. Direct Relationship eggs , cost M i l e a g e (mpg) Cost # eggs Units & Errors Inverse Relationship engine size , mpg engine size (L) 17 Practice Problems: 1. In 10 s a well trained sprinter weighing 100 lbs. runs 100 m. After a year of overeating the sprinter now weighs 250 lbs. Assuming that his weight is the only factor affecting his performance, calculate his new distance for a 10 s run. Show your steps in your calculations. 2. Using a regulation hardball weighing 150 grams, American league pitcher, Nolan Ryan, has delivered pitches clocked up to 180 km/h. Assuming ball weight to be the only factor affecting the speed of his pitch, calculate the top speed which this pitcher could throw a 4.5 kg bowling ball. 3. A liquid chemical storage tank can be filled in 15 minutes using a pump which transfers liquid at a rate of 120 L/min. Calculate a) the volume of the storage tank in litres and b) the number of minutes it would take to fill the tank using a pump which transfers 180 L/min. 4. Average adults have a lung capacity of 10 L at sea level (1.0 atmospheres pressure). Calculate the volume of the lungs when a skin diver dives to a depth at which the pressure increases to 2.5 atmospheres. Units & Errors 18 Solving Concentration Problems by Logical Statements: Problem: Calculate the grams of solute in 250 mL of 10%w/v KI soln. Solution: Start by writing out ‘what the given concentration unit means’. This is the first of the two logical statements: 10% w/v means: 100 mL soln. contains 10 g solute therefore: 250 mL 250 mL soln. contains x g solute = 10 g = 25 g KI 100 mL Problem: Calculate the concentration in g/kg for a soln. of 10 g HCl + 240 g H2O. Solution: 10 g HCl + 240 g H2O = 250 g soln. st 1 statement: 250 g soln. contains 10 g HCl 2nd statement: 1000 mL 1000 g soln. (1 kg) contains x g HCl = 10 g = 40 g/kg 250 mL Problem: Calculate the mass of KOH (MW = 56.1 g/ mol) to prepare 600 mL 0.45 M KOH Solution: 56.1 g 0.45 M KOH means: 1000 mL (1 L) contains 0.45 moles KOH = 25.2 g KOH 1 mol (Note this first calculation uses the unit factor method to convert moles to grams. This is valid because the quantity is unchanged; we are simply converting its units) 1st Statement: 1000 mL soln. contains 25.2 g KOH 2nd Statement: 600 mL 600 mL soln. contains x g KOH = 25.2 g = 15.1 g KOH 1000 mL Try these: 1. Calculate the %w/w of a soln. made with 20 g NaCl in 100 g H2O 2. Convert 50 g NaCl in 200 mL soln ( = 1.12 g/mL) to g/kg. 3. Calculate the mass of Na2CO3 (MW = 106 g/mol) in 150 mL of 2.0 M Na2CO3 soln. 4. Calculate the mass and vol. of 30.0% H2SO4 (=1.22 g/mL) that contains 50.0 g H2SO4 Answers: 1. 16.7 %w/w NaCl 2. 220 g/kg 3. 32 g Na2CO3 4. 167 g soln. and 137 mL soln. Units & Errors 19 Solving Dilution Problems by Logical Statements: Although dilution problems do not necessarily need two logical statements to solve, the calculation using ‘dilution factors’ is similar and uses the same reasoning skills. Some examples follow: Problem: A 5.0 mL aliquot from a 50 ppm Pb stock soln. is pipetted into a 25 mL volumetric flask and the flask is made up to the mark with water and mixed. Calculate the concentration of the final soln. Solution: The final solution is less concentrated, so we simply multiply the original concentration by a ‘dilution factor’, i.e., a ratio of the two volumes. 5 mL 25 mL Only two ratios are possible, either or . 25 mL 5 mL Of course we choose the first ratio (1/5) since makes the final concentration value lower than the original concentration. We know the final concentration is lower because a dilution was performed. dilution factor 5 mL 50 ppm = 10 ppm 25 mL Problem: A 20 g/mL Ni soln. was prepared by diluting 15 mL of a stock soln. to 50 mL. Calculate the concentration of the stock soln. Solution: 50 mL 20 g/mL Ni = 67 g/mL Ni 15 mL factor The ratio is set up so that the stock concentration will be greater than the diluted soln. concentration. Problem: 50 mg. Cl- is contained in 250 mL solution. How many mg Cl- are contained in a 10 mL aliquot of this solution. Solution: 10 mL 50 mg Cl- = 2 mg Cl250 mL or 250 mL solution contain 50 mg Cl- 10 mL = 2 mg Cl250 mL 10 mL solution contain x mg Cl- = 50 mg Cl- Try these: 1. 4 mL of a stock soln. was diluted to 100 mL. 5 mL of the diluted soln. contains 0.002 g F- Calculate the %w/v of F- in the stock soln. (answer = 1 % w/v) 2. 25 mL of a brine solution was diluted to 500 mL. From this 1st dilution, a 25 mL aliquot was diluted to 500 mL. A 20 mL aliquot of the 2nd dilution was titrated with an AgNO3 solution. The mass of Cl- as NaCl was determined to be 0.0350 g in the 20 mL aliquot that was titrated. Calculate the conc. (g/L) NaCl in the brine soln. (answer = 7.00 102 g/L) Units & Errors 20 Rearranging Equations 1. 2. 3. EH = m c T, solve for T T = T2 - T1, solve for T1 v2 = v1 + a t, solve for a Often we must rearrange an equation before we can solve for a term. We rearrange an equation so as to isolate the term to be solved for. By isolating a term we mean the term is alone, positive (+), and in the numerator on either side of the equation. Move an unwanted term to the opposite side of the equation by applying its reverse operation, then cancel to simplify. Multiplication is the reverse operation to division. Addition is the reverse operation to subtraction. 1. EH = m c T 3. v2 = v1 + a t (v2) - v1 = (v1 + a t) - v1 2. E H m c T mc mc EH T mc v2 -v1 = a t T = T2 - T1 (T) + T1 = (T2 -T1) + T1 T + T1 = T2 (T + T1) - T = (T2) -T T1 = T2 - T v2 v1 a t t t v2 v1 a t Note: In an equation, the whole left side = the whole right side. Any operation can be carried out on an equation without changing its equality so long as the same operation is applied to all terms on both sides. In the following equations, isolate and solve for the unknown where: L = loonie (100¢), Q = quarter (25 ¢), D = dime (10 ¢), and N = nickel ( 5 ¢). Wrong way: L 10 = 60 2 L + 10 = 60 2 L = 120 - 10 L 110 Units & Errors Right Way: L 10 60 2 ( 2L 10) 2 = (60) 2 L + 20 = 120 L = 120 - 20 = 100 21 Practice: Solve the following equations as indicated by rearranging the equations and isolating the desired term. Check your answers by substituting the coin values in for each letter. 1. Solve for N: 3. 5. 2 L 10 N Q 6 Solve for D: L = 3Q + 2D + N Solve for Q: Units & Errors 2 L 6Q 5 D D 2. Solve for L: L 5N Q 3 4. Solve for L: 1 6. Solve for Q: 5 N 3Q L L L 2 D 8 QN N QN Q 22 Scientific Notation - Answers Answers to Units Problems Page 1 6.8091 104 1a) 2a) 70 b) 2.3 10-5 b) 0.004098 c) 5.4 103 c) 83,000,000 d) 8.0 10-1 d) 0.000101 e) 5.04 10-2 Page 2 A B C D E common notation 440 710 1070 1105 1590 number of sig figs 2 2 3 4 3 scientific notation 4.4 102 7.1 102 1.07 103 1.105 103 1.59 103 A C common notation 442 1059 number of sig figs 3 4 scientific notation 4.42 102 1.059 103 Page 3 A B common notation 700 2300 number of sig figs 1 2 scientific notation 7 102 2.3 103 common notation 1.1 1.08 1.089 number of sig figs 2 3 4 scientific notation 1.1 100 1.08 100 1.089 100 Page 4 A B C Page 5 engine temp. (ºF) speed (km/h) common notation 183.7 97 number of sig figs 4 2 scientific notation 1.837 102 9.7 101 Page 6 a) 3 e) 5 i) 1 b) 2 f) 3 j) 3 c) 2 g) 4 d) 5 h) 4 Units & Errors 23 Scientific Notation - Answers Page 8 a) 2200 c) b) 2200 2300 e) 0.078 d) 2300 f) 0.077 2.5 103 mm Page 14 1. 2.0 105 dL 5. 1.98 lb 9. 2. 1.29 102 km 6. 4.56 105 ms 10. 8.42 10-6 kmol 3. 5.91 102 cs 7. 2 102 fm 11. 5.0 10-1 mol 4. 3.0 104 mL 8. 1.01 1011 g 12. 7.10 103 g/L Page 15 1. 4.49 leap years 3. 5.7 L/100 km 2. 2.0 10 cal. 4. 1.932 104 kg/m3 6 Page 18 1. 40 m 3. a) 1800 L, b) 10 min. 2. 6 km/h 4. 4L Units & Errors 24