Chem 106: Quiz 1
How many significant figures are contained in each of the following measurements? a) 38.7 g (b) 2 × 1018 m (c) 3,486,002 kg (d) 9.74150 × 10−4 J (e) 0.0613 cm3 (f) 17.0 kg (g) 0.01400 g/mL
A) 3 B) 4 C) 7 D)5 E)3 F)3 G)4
Explosion of a firecracker
Chemical Change
volume of a flu shot of measles
cubic centimeters
What is 'matter'? What are the different phases of 'matter'?
Anything that has mass and takes up space 1.gas 2. solid 3.liquid 4.plasma
Baking Soda
Compound
EN-1000.00
1.0 x 10^3
EN-22086
2.2 x 10^4
SF 0.239
3 sig figs (leading zeros do not count)
EN- 0.03344
3.3 x 10^-2
SF 0.05499
4 Sig Figs
SF 134.2
4 sig figs
Sig Figs 711.0
4 sig figs (trailing zeros)
SF 90743
5 sig figs
EN- 547.9
5.5 x 10^2
g) 0.000000738592
6 sig figs
EN- 0.0000000651
6.5 x 10^-8
EN-704
7.0 x 10^2
EN-0.007157
7.4 x 10^ -8
Physical Change
A change in a substance that does not involve a change in the identity of the substance
chemical change
A change in matter that produces one or more new substances
Mixture
A combination of two or more substances that are not chemically combined
Accuracy
A description of how close a measurement is to the true value of the quantity measured.
What is scientific Method?
A logical, systematic approach to the solution of a scientific problem
Element
A pure substance made of only one kind of atom
Pure Substance
A sample of matter, either a single element or a single compound, that has definite chemical and physical properties
Compound
A substance made up of atoms of two or more different elements joined by chemical bonds
Calculate these volumes. (a) What is the volume of 11.3 g graphite, density = 2.25 g/cm3? (b) What is the volume of 39.657 g bromine, density = 2.928 g/cm3?
A) 11.3/2.25= 5.02cm^3 B)39.657/2.298=13.54cm^3
The following quantities were reported on the labels of commercial products. Deter-mine the number of significant figures in each. (a) 0.0055 g active ingredients (b) 12 tablets 8 (c) 3% hydrogen peroxide (d) 5.5 ounces (e) 473 mL (f) 1.75% bismuth (g) 0.001% phosphoric acid (h) 99.80% inert ingredients
A) 2 B)2 c)1 D)2 E)3 F)3 G)1 H)4
Perform the following calculations and report each answer with the correct number of significant figures. (a)62.8 × 34 (b)0.147 + 0.0066 + 0.012 (c)38 × 95 × 1.792 9 (d)15 - 0.15 - 0.6155 (e)8.78 ×( 0.0500 / 0.478) (f)140 + 7.68 + 0.014 (g)28.7 - 0.0483 (h)(88.5 − 87.57) / 45.13
A) 2.1 x 10^3 B) 1.7 x 10 ^-1 C) 6.5 x 10 ^3 D) 1.4 x 10^1 E)0.918 F)1.5 x 10^2 G)28.7 H)0.02061
Calculate these masses. a)What is the mass of 6.00 cm3 of mercury, density = 13.5939 g/cm3? b)What is the mass of 25.0 mL octane, density = 0.702 g/cm3?
A) 6 x 13.5939= 81.6g B) 0.702 x 25 = 17.6g
Derived SI Unit
Any SI unit of measurement obtained from a combination of two or more SI base units.
Write down the formulae for 'Conversion of Temperature' among different units of temperature (°C,°F, K).
C to F = F 9/5 (c)+ 32 K to F= 9/5( K-273) + 32 F to C= 5/9(f-32) C to K= C = 273 K to C= k-273 F to K= 5/9 (f-32) + 273
Convert the boiling temperature of liquid ammonia, −28.1 °F, into degrees Celsius and kelvin
C=-33.4 K=240.K
Convert the temperature of the coldest area in a freezer, −10 °F, to degrees Celsius and kelvin.
C=23.3C K=249.7K
A substance composed of molecules each of which contains one hydrogen atom and one chlorine atom
Compound
What is the difference between Crystalline and Amorphous Solid?
Crystalline Solids are arranged in a repeating pattern Amorphous Solids are arranged in no order.
A substance composed of molecules each of which contains two iodine atoms
Element
Convert the temperature of dry ice, −77 °C, into degrees Fahrenheit and kelvin. 97.
F=-110F K=196K
Convert the boiling temperature of gold, 2966 °C, into degrees Fahrenheit and kelvin.
F=5371F K=3239K
My truck's gas mileage has dropped significantly, probably because it's due for a tune-up.
Hypothesis-tentative explanation of observation
Energy SI unit
Joule (J)
Temperature SI unit
Kelvin (K)
The mass of the moon
Kilograms (Kg)
(a) Falling barometric pressure precedes the onset of bad weather.
Law, Summarizing observations and describes them in some way of world
The pressure of a sample of gas is directly proportional to the temperature of the gas.
Law- summarizes the results (charles law)
Explain "Law of Conservation of Mass"?
Mass in an isolated system is neither CREATED nor DESTROYED by chemical reactions or physical transformations
The difference between "mass" & "weight"
Mass is how much matter an object has weight is how strong gravity pulls on the matter of a mass.
The distance from Dallas to Oklahoma city
Meter (m)
Baking Powder
Mixture
Gasoline
Mixture
Pancake Syrup
Mixture
AIR
Mixture of gases
Magnetizing of a Screwdriver
Physical
A sulfur atom and a sulfur molecule are not identical. What is the difference?
The sulfur atom is a single atom. The sulfur molecule is made up of more than one sulfur atom
All life on earth has evolved from a common, primitive organism through the process of natural selection.
Theory- Observing life and giving causes of natural selection; a law in nature
Sucrose
a compound that is the chief component of cane or beet sugar.
Precision
a measure of how close a series of measurements are to one another
homogeneous mixture
a mixture in which the composition is uniform throughout
extensive property
a property that depends on the amount of matter in a sample
intensive property
a property that depends on the type of matter in a sample, not the amount of matter
Is one Liter about an ounce, a pint, a quart, or a gallon
a quart= 0.94635 Liters
Complete the following conversions between SI units. (a) 612 g = ________ mg (b) 8.160 m = ________ cm (c) 3779 μg = ________ g (d) 781 mL = ________ L (e) 4.18 kg = ________ g (f) 27.8 m = ________ km (g) 0.13 mL = ________ L (h) 1738 km = ________ m (i) 1.9 Gg = ________ g
a) 612,000mg (1,000mg) b)816 cm (100 cm) c)0.003779 (1,000,000 ug) d)0.781 L (1000ml) e) 0.00418g (1g/0.001kg) F) 0.0278km (1m) g) 0.0013L (1000ml) H) 1,738,000m (1000m) I) 1.9 x 10 ^8 g (1 x 10^9 g)
Round off each of the following numbers to two significant figures: (a) 0.436 (b) 9.000 (c) 27.2 (d) 135 (e) 1.497 × 10−3 (f) 0.445
a)0.44 b)9.0 c)27 d)140 e)0.0015 f)0.45
SF 10000
ambiguous
uncertainty
an estimate of how much a measured or calculated value differs from a true value
mass of a textbook
certain (one textbook)
the number of cm in 2 cm
certainty
Burning of Gasoline
chemical change
Souring of Milk
chemical change
coal burning
chemical change
Mercury Oxide
compound
water
compound
mass of a dozen eggs
degree of uncertainty
Nitrogen
element
Sulfur
element
iron
element
oxygen
element
copper
element on the periodic table
# of eggs in basket
exactly
At a higher temperature, solids (such as salt or sugar) will dissolve better in water.
hypothesis
Alcohol burning
kelvin (k)
Density SI unit
kg/m^3
Density of air
kg/m^3
mass SI unit
kilogram (kg)
the speed of sound
km/s
Volume SI unit
m^3
number of gallon necessary to fill an automobile tank
measured w degree of certainty
Length SI unit
meter (m)
Heterogenous
not similar; very different; mixed together
Is a meter about an inch, a foot, a yard , or a mile
one meter= 39.37 inches = 3.28 feet = 1.09 yards about a yard
Condensation of Steam
physical change
dissolving sugar in water
physical change
ice melting
physical change
melting of gold
physical change
mixing chocolate syrup into milk
physical change
Physical and Chemical Properties
physical properties are unique for a particular substance and include color, density, melting point and boiling point. chemical properties relate to how a substance interacts with another substance ( reactivity, Flammability, oxidization states)
Time SI unit
s (seconds)
the area of the state of deleware
square meter
What is chemistry?
the study of the composition of matter and the changes that matter undergoes
Matter consists of tiny particles that can combine in specific ratios to form sub-stances with specific properties.
theory
The time required to drive from San Francisco to Kansas City at an average speed of 53 mi/h
uncertain
