Chem 106: Quiz 1

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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


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