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Quick Mid Term Review. Multiple Choice Questions! . Which of the following is not a pure substance?. water carbon dioxide carbon d. air. Solutions may be. solids. liquids. gases. d. All of the above. Explain the difference between a scientific law (X) and a scientific theory (Y).

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quick mid term review

Quick Mid Term Review

Multiple Choice Questions!

solutions may be

Solutions may be

solids.

liquids.

gases.

d. All of the above

explain the difference between a scientific law x and a scientific theory y

Explain the difference between a scientific law (X) and a scientific theory (Y).

X = is proven; Y = is not proven

X = is not proven; Y = is proven

X = tells what happens; Y = explains why things happen

X = explains why things happen; Y = tells what happens

properties that describe the way a substance reacts to form other substances are called

Properties that describe the way a substance reacts to form other substances are called

physical properties.

chemical properties.

homogeneous properties.

d. heterogeneous properties.

when nitric acid is mixed with copper metal a brown gas forms this is an example of

When nitric acid is mixed with copper metal, a brown gas forms. This is an example of

an accident.

a chemical reaction.

a physical property.

d. an extensive property.

heat flows from an object

Heat flows from an object

at high temperature to an object at low temperature.

at low temperature to an object at high temperature.

to another object at the same temperature.

d. at high elevation to an object at low elevation.

the nucleus of an atom contains

The nucleus of an atom contains

protons and neutrons.

protons and electrons.

electrons and neutrons.

d. air.

two atoms with the same atomic number but different mass numbers are called

Two atoms with the same atomic number but different mass numbers are called

mutants.

isomers.

isotopes.

d. symbiots.

the elements found on the left side of the periodic table tend to electrons

The elements found on the left side of the periodic table tend to ______ electrons.

gain

lose

keep

d. share

a metal and a nonmetal react to form compound

A metal and a nonmetal react to form ________ compound.

a molecular

a mixed

an empirical

d. an ionic

compounds composed only of carbon and hydrogen are called

Compounds composed only of carbon and hydrogen are called

binary acids.

carbohydrates.

hydrocarbons.

d. alkanes.

which of the formulas below does not represent a compound that actually exists

Which of the formulas below does not represent a compound that actually exists?

CaCO3

H2O2

KMnO4

d. Na2PO3

naocl is named

NaOCl is named

sodium chlorate.

sodium chlorite.

sodium perchlorate.

d. sodium hypochlorite.

lino 3 is named

LiNO3 is named

lithium nitrate.

lanthanum nitrate.

lanthanum nitrite.

d. lithium nitrite.

cl 2 o 7 is named

Cl2O7 is named

chlorine(VII) oxide.

dichlorine hexaoxide.

dichlorine heptaoxide.

d. bichlorine heptaoxide.

hydrocarbons burn to form

Hydrocarbons burn to form

H2O and CO2.

charcoal.

methane.

d. O2 and H2O.

c 6 h 6 o 2 co 2 h 2 o when this equation is correctly balanced the coefficients are

C6H6 + O2 CO2 + H2OWhen this equation is correctly balanced, the coefficients are

1, 7  6, 3.

1, 8  6, 3.

2, 15  12, 6.

d. 2, 16  12, 6.

2 nan 3 2 na 3 n 2 this is an example of a reaction

2 NaN3 2 Na + 3 N2This is an example of a _______ reaction.

decomposition

combination

combustion

d. replacement

slide21

Ribose has a molecular weight of 150 grams per mole and the empirical formula CH2O. The molecular formula of ribose is

C4H8O4.

C5H10O5.

C6H14O4.

d. C6H12O6.

a homogeneous mixture of two or more components is referred to as

A homogeneous mixture of two or more components is referred to as

a solute.

a solution.

an electrolyte.

d. a mess.

the solvent in a sample of soda pop is

The solvent in a sample of soda pop is

sugar.

carbon dioxide.

water.

d. air.

when fe no 3 2 dissolves in water the particles in solution are

When Fe(NO3)2 dissolves in water, the particles in solution are

Fe+ and (NO3)2-.

Fe2+ and 2 NO3-.

Fe and 2 NO3.

d. Fe and N2 and 3 O2.

as a helium filled balloon rises its volume increases this is an example of law

As a helium-filled balloon rises, its volume increases. This is an example of _______ Law.

Avogadro’s

Boyle’s

Charles’s

d. Gay-Lussac’s

avogadro s law states that the volume of a sample of a gas is proportional to the of the gas

Avogadro’s Law states that the volume of a sample of a gas is proportional to the _______ of the gas.

number of moles

mass

pressure

d. temperature

standard temperature and pressure stp equals x atmosphere s and y degrees celsius

Standard temperature and pressure (STP) equals (X) atmosphere(s) and (Y) degrees Celsius.

X = 0, Y = 25

X = 1, Y = 0

X = 1, Y = 25

d. X = 0, Y = 0

a sample of 2 0 moles of nitrogen n 2 gas at stp occupies a volume of liters

A sample of 2.0 moles of nitrogen (N2) gas at STP occupies a volume of _______ liters.

11.2

22.4

44.8

d. 89.6

the partial pressure of each gas in a mixture of gases is proportional to the of the gas

The partial pressure of each gas in a mixture of gases is proportional to the _______ of the gas.

mass

molecular weight

square root of the molecular weight

d. mole fraction

kelvin temperature celsius temperature number of moles d pressure

The kinetic-molecular theory of gases states that the average kinetic energy of the gas particles is proportional to the _______ of the gas.

Kelvin temperature

Celsius temperature

number of moles

d. pressure

neon gas undergoes effusion krypton gas does

Neon gas undergoes effusion _______ krypton gas does.

slower than

at the same rate as

twice as fast as

d. four times as fast as

a gas is most likely to exhibit ideal behavior at x temperature and y pressure

A gas is most likely to exhibit ideal behavior at (X) temperature and (Y) pressure.

X = low, Y = low

X = low, Y = high

X = high, Y = low

d. X = high, Y = high

the rate of a reaction can be increased by

The rate of a reaction can be increased by

increasing reactant concentrations.

increasing the temperature.

adding a suitable catalyst.

d. All of the above

over time the rate of most chemical reactions tends to

Over time, the rate of most chemical reactions tends to _______.

increase

decrease

remain constant

d. oscillate

slide37

If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.

zeroth

first

second

d. third

reaction a b c d rate k a b the overall order of this reaction is

Reaction: A + B  C + DRate = k[A][B]The overall order of this reaction is

first.

second.

third.

d. fourth.

reaction w x y z rate k w the order of this reaction with respect to x is

Reaction: W + X  Y + ZRate = k[W]The order of this reaction with respect to X is

zeroth.

first.

second.

d. third.

slide40

The time required for the concentration of a reactant to be reduced to half of its initial value is called the

midpoint of the reaction.

equivalence point of the reaction.

half-rate of the reaction.

d. half-life of the reaction.

the rate determining step is the step in a reaction mechanism

The rate-determining step is the _______ step in a reaction mechanism.

first

last

c. fastest

d. slowest

adding a catalyst increases the rate of a chemical reaction because the presence of the catalyst

Adding a catalyst increases the rate of a chemical reaction because the presence of the catalyst

increases molecular velocities.

increases molecular collisions.

decreases energy of activation.

d. All of the above

at equilibrium the rate of the forward reaction is the rate of the reverse reaction

At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.

equal to

slower than

faster than

d. the reverse of

the reaction quotient q is usually represented by

The reaction quotient Q is usually represented by

[reactants] / [products].

[products] / [reactants].

[reactants]  [products].

d. [reactants] + [products].

if the value of the equilibrium constant is large then will mostly be present at equilibrium

If the value of the equilibrium constant is large, then _______ will mostly be present at equilibrium.

reactants

products

catalysts

d. shrapnel

q the reaction quotient k the equilibrium constant at equilibrium which is true

Q = the reaction quotientK = the equilibrium constantAt equilibrium, which is true?

Q > K

Q < K

Q = K

d. Q2 = K

slide47

CO2 + H2 CO + H2OIf all species are gases and H2 is added, the concentration of CO at equilibrium will

increase.

decrease.

remain unchanged.

d. disappear.

co 2 h 2 co h 2 o if all species are gases and h 2 o is added the equilibrium concentration of co

CO2 + H2 CO + H2OIf all species are gases and H2O is added, the equilibrium concentration of CO

will increase.

will decrease.

will remain unchanged.

d. will disappear.

co 2 h 2 co h 2 o if all species are gases and co 2 is removed the co at equilibrium will

CO2 + H2 CO + H2OIf all species are gases and CO2 is removed, the [CO] at equilibrium will

increase.

decrease.

remain unchanged.

d. disappear.

co 2 h 2 co h 2 o increasing the temperature of this endothermic reaction will co at equilibrium

CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.

increase

decrease

not change

d. eradicate

co 2 h 2 co h 2 o if all species are gases and the container is compressed the amount of co will

CO2 + H2 CO + H2OIf all species are gases and the container is compressed, the amount of CO will

increase.

decrease.

remain unchanged.

d. vanish.

co 2 h 2 co h 2 o adding a catalyst to this reaction will cause the co at equilibrium to

CO2 + H2 CO + H2OAdding a catalyst to this reaction will cause the [CO] at equilibrium to

increase.

decrease.

remain unchanged.

d. cease to exist.