H CH 1 HOMEWORK:
Misc:
1. Identify the SI unit and prefix that would be most appropriate for measuring the
following:
a) the length of a pencil.
mm, cm, m
b) The width of the classroom
m
c) The diameter of the graphite in a pencil
mm
d) The distance from here to Meyersdale
km
e) The mass of a person
kg
f) The mass of a grape
g
g) The volume of a glass of water
mL, cL, L
h) The volume of a dump truck load of sand. m3
2. Determine the number of significant digits in each of the following:
a)
b)
c)
d)
e)
f)
g)
65.42 4
385
3
.014
2
709.2 4
5006.12 6
400
1
260.
3
h) 0.47
i) 0.0068
j) 7.0
k) 36.00
l) .0070
m) 100.6040
n) 340.00
2
2
2
4
2
7
5
3. Round off the following measurements to the indicated amount of significant digits:
a)
b)
c)
d)
e)
2.68 to 2 sig figs
457.26 to 3 sig figs
.00254 to 1 sig fig
27 to 1 sig figs
.112504 to 5 sig figs
2.7
457
.003
30
.11250
SCIENTIFIC NOTATION
Write the following numbers in scientific notation. Round to 2 numbers after the
decimal.
1. 100
1.0 x 102
6. .024
2.4 x 10-2
2. 10500
1.05 x 104
7. .00000458 4.58 x 10-6
3. –800
-8.00 x 102
8. -.6
-6 x 10-1
4. 6
6 x 100
9. -.00054
–5.4 x 10-4
5. –216000
-2.16 x 105
10. .00110
1.10 x 10-3
Rewrite the following in expanded notation.
11. 4.2 x 102
420
16. 4.82 x 10-1 .482
12. –8.43 x 106
-8 430 000
21. 14.86
1.49 x 101
24. 1486.2 x 106 1.49 x 109
22. 128.4
1.28 x 102
25. 1486.2 x 10-6 1.49 x 10-3
23. 13.0
1.3 x 101
17. –9.02 x 10-6
-.000 009 02
13. 4.8 x 103
4800
18. 5.77 x 10-4
.000 577
14. –1.97 x 1012
-1 970 000 000 000
19. 8.4 x 10-10
.000 000 000 84
15. 7.14 x 105
714 000
20. 3.00 x 10 –2
.03
Write the following numbers in scientific notation. Round to 2 numbers after the
decimal.
List of numbers (comparison)…planets
PERFORM THE FOLLOWING CALCULATIONS USING SIG FIGS.
1. 112.34 + 23.3 =
135.6
2. 1320 – 212 =
1110
3. 14.55423 + 112.232 + 1.01 =
127.80
4. 10000 – 8 =
10000
5. 110. + .0987 =
110.
6. 23.1 x 1.8 =
42
7. 112.0 x 10 =
1000
8. 1129.10 / 2.000 =
564.6
9. 100 x 23 =
2000
10. 76.54 x 1.82 x 12.552427 =
1750
11. (34.98 + 2.3) / 2.86 =
13.0
12. 9.10 x 2.7762 + 1.23 =
26.5
13. (6.78 + 2.4333 – 3.7) =
2.0
2.8
14. (.0098 + 1.009) x (2.978 + .00725) =
3.042
15. 1/3 =
.3
600./3.0 =
DENSITY
Show all work and round to the correct number of sig figs.
Consider the following list of elements:
Barium
Copper
Germanium
Platinum
Gold
Aluminum
Sulfur
Calcium
Nickel
Magnesium
1. List the elements in order of increasing density.Ca, Mg, S, Al, Ba, Ge, Ni, Cu, Au, Pt
2. Which of the above elements would float in Bromine? Ca, Mg, S, Al
3. How many cm3 is 6.2 x 103 g of lithium? 12000 cm3
4. How many cm3 is 841 g of silver?
80.1 cm3
5. What mass of Uranium is 95 cm3 of Uranium? 1800 g
6. How many grams would be in 1280 cm3 of Mercury? 17300 g
7. A student determines the volume of a sample of iron to be 11.0 cm3. Its mass is 93.21
g.
a. Calculate the experimental density of Iron.
8.47 g/cm3
b. Calculate the experimental error. (No sig figs)
.6 g/cm3
c. Calculate the percent error. (No sig figs)
7.62 %
8. A glass of wine is mainly water and ethanol (about 10% by volume). If a cup of wine
is poured, what is the mass of the wine? The density of ethanol is .79 g/mL
231.53g review…..
9. What are the dimensions of a cube holding 250g of water? No sig figs 6.3 cm
10. If the specific gravity of carbon tetrachloride is 1.6, what is the mass of 25 ml of
carbon tetrachloride? No sig figs
40 g
WATER VAPOR PRESSURE:
TEMP (C)
PRESSURE (mmHg)
0.0
5.0
10.0
12.5
15.0
17.0
20.0
 Find the slope
 What is the pressure at 8 C?
What is the pressure at 25 C?
4.6
6.5
9.2
10.9
12.8
14.7
17.5
.64 mmHg/C
8.73 mmHg
19.62 mmHg
DENSITY OF WATER:




TEMP (C)
DENSITY (g/ml)
4
6
8
10
20
30
40
.99997
.99994
.99985
.99970
.99820
.99565
.99222
Find the slope
-.0002 g/mL/C
Find the density at 25 C
.99621 g/mL
What information does the slope provide?
How are the variables related?
Inversely
DIMENSIONAL ANALYSIS:
English – English:
1. How many ounces are in 2 pounds?
32 oz
2. Change 13 inches to feet. 1.08 ft
3. 32 inches would be how many yards?
.89 yds
4. If there are 2 pints in a quart and 4 quarts in a gallon, how many pints are in 2.2
gallons? 17.6 pints
Metric – Metric:
5. How many meters are in 1500 mm?
6. Change 740 cL to hL.
1.5 m
.074 hL
7. 1.4 x 104 g would be how many Mg?
.014 Mg
8. 1100 nm would be how many pm?
1.1 x 106 pm
Metric – English/English – Metric:
9. A 3 mile walk is how many km? 4.83 km
10. 254 mm is how many inches?
10 in
11. 10 gallons would be how many L?
37.84 L
12. 635 pounds would be how many kg?
288.29 kg
Dimensional Analysis II:
1. An average car has a fuel efficiency of about 25 miles/gal. If we are selling the car in
Europe, what would be the efficiency in km/L?
10.6 km/L
2. 87 cm2 would be how many in2?
13.49 in2
3. A typical home faucet has a volumetric flow rate of about 3.2 gal/min. What would
that rate be in L/s? Watch sig figs.
.20 L/s
4. A 1 gallon container is how many ft3?
.13 ft3
5. 470 cL would be how many quarts? Watch sig figs.
5.0 qts
6. A typical mass flow rate for production of polystyrene from a single plant is about
2.12 tons/day. How many Mg is that in a year?
702.6 Mg/yr
7. If you need 27 square yards of carpeting for a room that is square, what would be the
dimensions of the room in meters?
4.75 m
8. 6101 in3 would be how many m3? Watch sig figs.
.100 m3
9. A large river flows at 2.6 x 105 gal/s into a loch that is 75 m x 30 m x 18 m. How long
will it take to fill the loch? 41.16 s
10. A city uses 7 million gallons of water in a day. How many tons of water is that in a
year? 1.06 x 107 tons/yr
go back and do #8 from Density HW
HEAT AND TEMPERATURE:
1. Perform the following conversions:
12.4C = 54.3 F
76.4F = 24.7 C
246 K = -27 C
220F = 377.5 K
2500 J = 6.0 x 102 cal (SF)
56 kcal = 234 kJ
2. A heating coil is placed into 300 g of water at 25C. After 3 minutes the temperature
of the water is 50.C. The specific heat of water is 4.184 J/g • C. How much heat
did the water absorb?
31380 j
3. 2 oz of gold are to be melted down for use in making jewelry. How much heat would
be required to heat this gold from 30 C to its melting point of 1064 C?
7569.7 j
4. It takes 75000 J of energy to change 500.00 g of an unknown substance from 25.0C
to 90.0C. What is the specific heat of the substance? (SF)
2.3 j/g C
5. A mass of 1200 g of water has a temperature of 22.0C. What will the new
temperature of the water be if 10000 J of energy is absorbed by the water? (SF)
24 C
6. What mass of copper can be increased in temperature by 80 C with 3000 cal of
energy? 407.53 g
7. If a piece of aluminum with a mass of 3.90 g and a temperature of 99.3 C is dropped
into 10 cm3 of water at 22.6 C, what will the final temperature of the system be?
28.54 C
8. If a piece of cadmium with a mass of 65.6 g and a temperature of 100.0  C is
dropped into 25.0 cm3 of water at 23.0 C, what will be the final temperature of the
system? 32.8 C
9. A piece of unknown metal with a mass of 23.8 g is heated to 100.0 C and dropped
into 50 ml of water at 24.0 C. The final temperature of the system is 32.5 C. What
is the specific heat of the metal? 1.106 j/g C
10. A typical hot water heater can hold 40 gallons of water.
a) If the height of the heater can be no more than 2 m, then what would be the smallest
possible diameter of the heater? (assume it is cylindrical)
.31 m
b) If the mass of the empty heater is 110 kg, what would the mass of the full heater be?
261.36 kg
c) If the incoming water has an initial temperature of 60 F, how much heat would be
required to heat the full tank of water to 115 F?
1.93 x 107 j
CH 1 Review:
1. What would the SI unit for area be?
List several possible units for volume.
m2
L, mL, cm3
2. What is the relationship between cm3 and ml? Same value, equivalent
3. What is meant by the density of a material?
The ratio of mass to volume
4. What is the rule governing the number of sig figs in calculations involving addition
and subtraction? Multiplication and division? Column rule
Least amount rule
5. What is meant by an exact conversion factor? Give two examples.
2 values that are defined as being equivalent. Eg; 1 ft = 12 in, 100 cL = 1 L
6. How many sig figs are in each of the following:
34.110 5
.0098 2
1009 4
1200 2
7. Convert the following:
a) 12 C to F 53.6 F
b) 123 F to K 323.6 K
8. a) 25 cal would be how many j? 104.6 j
b) 6.5 kj would be how many cal? 1553 cal
9. Determine the specific heat of a substance if a 25 g sample absorbed 34 j as it was
heated from 21 C to 33 C.
.113 j/g C
10. Convert the following:
a) 24.89 kg to pg 2.49 x 1016 pg
b) 223 ml to gal .059 gal
11. A piece of copper is 12 cm long by 8.5 cm wide and .5 cm thick. What is the mass of
the copper?
457 g
12. Perform the following calculations using the rules for significant figures:
a) 4.07 + 1.863
5.93
b) 3127.55 – 784.2
2343.4
c) 9.40 x 2.6
24
d) 1.50/2
.8
13. Identify the following as endothermic or exothermic:
a) melting ice
endothermic
b) burning charcoal
exothermic
c) photosynthesis
endothermic
d) water evaporating
endothermic
14. B
15. Why is it important to make temperature change come out as a positive value when
performing specific heat problems? No such thing as negative energy or negative mass
16.
Aluminum has a specific heat more than twice that of copper. Identical masses of
aluminum and copper, both at 0C, are dropped simultaneously into the same can of hot
water. When the system has come to thermal equilibrium:
A) the aluminum is at higher temperature than the copper
B) the copper is at higher temperature than the aluminum
C) the aluminum and copper are at the same temperature
C
17. E
A
18. Choose 1 of the 6 following scenarios.