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Chemistry Sem 2 Final Review

Total questions: 80

Worksheet time: 40mins

Name
Class
Date
1.
Which of the following is true of chemical reactions?
a)
Only physical changes occur.
b)
New substances must form.
c)
A change of state must occur.
d)
The chemical properties of the reactants must be the sames as the products.
2.
A substance that is formed by a chemical reaction is called a...
a)
mole
b)
product
c)
coefficient
d)
reactant
3.
A substance that enters into a chemical reaction is called a...
a)
mole
b)
product
c)
coefficient
d)
reactant
4.
Which of the following is the correct formula for magnesium reacts with chlorine to produce magnesium chloride.
a)
Mg -->Cl₂ + MgCl₂
b)
MgCl₂ --> Mg + Cl₂
c)
MgCl + Cl --> MgCl₂
d)
Mg + Cl₂ --> MgCl₂
5.
In a chemical reaction what is the relationship between the mass before a reaction and after the reaction?
a)
They masses must be equal
b)
The mass of the products must be greater than the mass of the reactants.
c)
The mass of the reactants must be greater than the mass of the products.
d)
There is no relationship to mass.
6.
How many oxygen atoms are there in 2Ca(NO3)2?
a)
4
b)
6
c)
10
d)
12
7.
What coefficient needs to be added to sodium to balance Na + MgCl2 --> NaCl + Mg
a)
1
b)
2
c)
3
d)
4
8.
What is the general formula for a double replacement reaction?
a)
A + B --> AB
b)
AB --> A + B
c)
A + BX --> AX + B
d)
AX + BY --> AY + BX
9.
What kind of reaction is C2Cl4 + Cl2 --> C2Cl6
a)
Direct Combination (synthesis)
b)
Decompostion
c)
Single Replacement
d)
Double Replacement
e)
Combustion
10.
What coefficient needs to be added to oxygen to balance 4Al + O2 --> Al2O3
a)
1
b)
2
c)
3
d)
4
11.
One amu is based as the mass of which atomic nucleus?
a)
hydrogen-1
b)
carbon-12
c)
carbon-14
d)
oxygen-16
12.
Which of the following is a diatomic element?
a)
sodium
b)
chlorine
c)
neon
d)
sulfur
13.
Avogadro's number
a)
the mass of a proton in a particular nucleus.
b)
6.022E23
c)
22.4 liters
d)
The mass in grams of one mole of substance.
14.
The mass of 6.022E23 particles of a particular substance is called...
a)
atomic mass
b)
molar volume
c)
molar mass
d)
formula mass
15.
At the same temperature and pressure, equal volumes of different gasses contain...
a)
equal numbers of particles
b)
different numbers of particules
c)
equal masses
d)
equal molar masses
16.
What is standard temperature?
a)
373 K
b)
100 C
c)
20 C
d)
273 K
17.
The ratio of the element mass to the mass of the compound is called...
a)
molar mass
b)
molar volume
c)
percent composition
d)
empirical mass
18.
The simplest whole-number ratio of the atoms of each element in a compound.
a)
formula mass
b)
structural formula
c)
empirical formula
d)
molecular formula
19.
The actual number of atoms of each element in a compound.
a)
formula mass
b)
structural formula
c)
empirical formula
d)
molecular formula
20.
Stoichiometry can tell us...
a)
if a reaction is possible
b)
new and missing elements
c)
the amount of product that should form
d)
if a compound is toxic
21.
Which term describes the number of particles in 1 mole?
a)
Avogadro's number
b)
Dalton's number
c)
Lavoisier's number
d)
Boyle's number
22.
In a balanced chemical equation, the molar ratio is determined from...
a)
the number of atoms in the compound
b)
the coefficients in the equation
c)
the molar mass of the compounds
d)
the molecular volume of the gases
23.
What is standard pressure?
a)
The pressure of a gas at room temperature.
b)
22.4 liters
c)
760 atm
d)
101.3 kPa
24.
What is the volume of one mole of gas at STP?
a)
6.022E23 mL
b)
22.4 liters
c)
760 atm
d)
It depends on the type of gas.
25.
The limiting reactant in a chemical reaction will be the substance...
a)
that is left over.
b)
that is used up.
c)
with the greatest mass prior to the reaction.
d)
with the least mass prior to the reaction.
26.
The percent yield of product in a chemical reaction is defined as the ratio of...
a)
expected yield to actual yield.
b)
actual yield to empirical yield.
c)
actual yield to expected yield.
d)
expected yield to theoretical yield.
27.
Exothermic reactions are reactions that...
a)
release heat.
b)
absorb heat
c)
always produce flames.
d)
are very rare.
28.
Endothermic reactions are reactions that...
a)
release heat.
b)
absorb heat
c)
always produce flames.
d)
are very rare.
29.
What is the SI unit for heat?
a)
Celsius
b)
Kelvin
c)
Calories
d)
Joules
30.
What is the heat capacity per gram of a substance?
a)
Entropy
b)
heat capcity
c)
BTUs
d)
Specific heat
31.
The energy of a phase change where a solid becomes liquid.
a)
heat of fusion
b)
heat of vaporization
c)
heat capacity
d)
Specific heat
32.
The amount of heat needed to raise the temperature of an object by 1 K.
a)
heat of fusion
b)
heat of vaporization
c)
heat capacity
d)
Specific heat
33.
Which of the following is NOT a property of gases?
a)
Easily compressed
b)
diffusion
c)
exerts pressure equally in all directions
d)
massless
34.
If we raise the temperature of a gas in a fixed volume container, what change will occur?
a)
Number of particles will change.
b)
The density will change
c)
the pressure will change
d)
the number of moles will change.
35.
The ability of gases to spread rapidly through other gases is due to...
a)
inelastic collisions in gas particles.
b)
the high density of gases.
c)
the slow motion of gas particles.
d)
the large space between particles and Brownian motion.
36.
To describe the conditions of a gas, which of the following is NOT needed?
a)
Pressure
b)
Density
c)
Temperature
d)
Volume
37.
According to Boyle's Law, if the temperature of a gas remains constant the pressure and volume are _?_.
a)
constant
b)
directly proportional
c)
inversely proportional
d)
independent
38.
According to Charles' Law; if the pressure of a gas remains constant the volume and absolute temperature are...
a)
constant
b)
directly proportional
c)
inversely proportional
d)
independent
39.
Which of the following formulas would be used to find the pressure of a mixture of different gases?
a)
Ideal Gas Law: PV=nRT
b)
Boyle's Law: PV = P'T'
c)
Gay-Lussac's Law: P/T = P'/T'
d)
Dalton's Law: P = P₁ + P₂ + P₃...
40.
When working with the gas laws, temperatures...
a)
must be in Fahrenheit.
b)
must be in Celsius.
c)
must be in Kelvin.
d)
can be in any unit as long as you are consistent.
41.
The ideal gas law will not apply to gasses with...
a)
high temperatures or low pressures
b)
high pressures or low temperatures
c)
low densities
d)
The Ideal Gas Law always works.
42.
Molarity is defined as the ratio of...
a)
moles of solvent/liters of solute
b)
moles of solute/ kilograms of solvent
c)
moles of solute/liters of solution
d)
moles of solute/moles of solvent
43.
Molality is defined as the ratio of...
a)
moles of solvent/liters of solute
b)
moles of solute/ kilograms of solvent
c)
moles of solute/liters of solution
d)
moles of solute/moles of solvent
44.
An Arrhenius acid is any acid which...
a)
has a pH lower than 7.
b)
dissociates in water to form hydrogen ions.
c)
dissociates in water to form hydroxide ions.
d)
has a pH higher than 7.
45.
An Arrhenius base is any base which...
a)
has a pH lower than 7.
b)
dissociates in water to form hydrogen ions.
c)
dissociates in water to form hydroxide ions.
d)
has a pH higher than 7.
46.
The word "acid" is actually derived from that taste of an acid which is best described as...
a)
sweet
b)
bitter
c)
sour
d)
salty
47.
Which taste is usually associated with bases?
a)
sweet
b)
bitter
c)
sour
d)
salty
48.
An ionic compound that forms in the neutralization reaction between an acid and a base is called a(n)...
a)
indicator
b)
hydronium ion
c)
hydroxide ion
d)
salt
49.
A substance that changes color due to changes in pH is called a(n)...
a)
indicator
b)
hydronium ion
c)
hydroxide ion
d)
salt
50.
A Bronsted-Lowry Base is a base which can...
a)
donate hydrogen ions.
b)
have a pH less than 7
c)
absorb hydrogen ions.
d)
produce hydronium.
51.
Which of the following is true about pure water?
a)
all of these are true.
b)
it can produce hydronium.
c)
it can produce hydroxide
d)
it is neutral on the pH scale
e)
it is a weak acid
52.
The definition of pH is...
a)
[c base][hydronium]/[acid]
b)
-log[hydronium]
c)
-log[hydroxide]
d)
[c acid][hydroxide]/[base]
53.
What is true about a strong acid versus a weak acid?
a)
Strong acids dissolve more things.
b)
Strong acids are more concentrated.
c)
Strong acids are more ionized.
d)
Strong acids have more hydrogens in their formulas.
54.
Which of the following statements is NOT true?
a)
Strong or weak in acids and bases has nothing to do with concentration.
b)
A dilute strong acid can have the same number of ions as a concentrated weak acid.
c)
Strong and weak mean the same thing as concentrated or dilute.
d)
Some weak acids/bases can dissolve a large number of solutes.
55.
A substance which helps keep the pH constant by absorbing and releasing ions.
a)
Indicator
b)
Arrhenius Acid
c)
Arrhenius Base
d)
Buffer
56.
Which neutralization reaction is most likely to form a neutral salt?
a)
Strong acid and strong base
b)
Strong acid and weak base
c)
Weak acid and strong base
d)
Weak acid and weak base
57.
Which of the following is not a carbon allotrope?
a)
Graphite
b)
Amorphous carbon (coal)
c)
Diamonds
d)
Alkanes
58.
What is an alkane?
a)
A saturated hydrocarbon.
b)
A hydrocarbon with at least one double covalent bond.
c)
A hydrocarbon with at least one triple covalent bond.
d)
A hydrocarbon without any branches.
59.
What family of hydrocarbons does 2,3,4-trimethyldecane belong to?
a)
Alkane
b)
Alkene
c)
Alkyne
d)
Hydrocarbon derivative
60.
What family of hydrocarbons does 2,3-heptadiene belong to?
a)
Alkane
b)
Alkene
c)
Alkyne
d)
Hydrocarbon derivative
61.
Which of the following cannot be the proper name of a branched alkane?
a)
2,2-dimethyloctane
b)
2-ethylpentane
c)
2,2,3,3-tetramethylhexane
d)
5-propyldecane
62.

Which of the following best describes a catalyst in a chemical reaction?

a)

It is consumed during the reaction.

b)

It increases the amount of product formed.

c)

It speeds up the reaction without being used up.

d)

It changes the reactants into different elements.

63.

What is the term for the minimum amount of energy required to start a chemical reaction?

a)

Potential energy

b)

Bond energy

c)

Activation energy

d)

Kinetic energy

64.

Which of the following is NOT a property of gases according to the kinetic molecular theory?

a)

Gas particles have negligible volume compared to the container.

b)

Collisions between gas particles are elastic.

c)

Gas particles are in constant, random motion.

d)

Gas particles attract each other strongly.

65.

Which law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases?

a)

Avogadro's Law

b)

Charles' Law

c)

Dalton's Law

d)

Boyle's Law

66.

What is the term for the reactant that determines the maximum amount of product that can be formed in a chemical reaction?

a)

Catalyst

b)

Limiting reactant

c)

Excess reactant

d)

Product

67.

Which of the following best describes an endothermic reaction?

a)

Occurs only at high temperatures

b)

Absorbs heat from the surroundings

c)

Releases heat to the surroundings

d)

Produces light

68.

Which of the following best describes a decomposition reaction?

a)

A compound reacts with oxygen to produce energy.

b)

Two compounds exchange ions to form two new compounds.

c)

Two elements combine to form a compound.

d)

A single compound breaks down into two or more simpler substances.

69.

What is the product when sodium hydroxide reacts with hydrochloric acid?

a)

Hydrogen gas and sodium oxide

b)

Sodium and chlorine gas

c)

Sodium hydroxide and hydrochloric acid

d)

Sodium chloride and water

70.

Which of the following best describes a decomposition reaction?

a)

A substance reacts with oxygen to produce energy.

b)

A single compound breaks down into two or more simpler substances.

c)

Two compounds exchange ions to form two new compounds.

d)

Two elements combine to form a compound.

71.

Which law states that mass is neither created nor destroyed in a chemical reaction?

a)

Law of Constant Composition

b)

Law of Definite Proportions

c)

Law of Multiple Proportions

d)

Law of Conservation of Mass

72.

Stoichiometry is...

a)


The study of reaction rates.

b)

Mole to mole conversions

c)


the quantitative relationships in a chemical reaction.

d)

the study of expected yields.

73.

The expected or theoretical yield is...

a)

the amount of product predicted by stoichiometric calculations

b)


the amount of product actually produced in a reaction.

c)


the sum of the reactants masses.

d)

always smaller than the mass of one reactant.

74.

In the reaction: 2 H₂ + O₂ --> 2 H₂O... what is the mole ratio of oxygen to water?

a)

2:2

b)

1:2

c)

3:2

d)

2:1

75.

The ratio of the mass of the individual elements to the mass of the compound.

a)


Percent composition

b)


Empirical Formula

c)

Molecular Formula

d)


Structural Formula

76.

1 mol = ?

a)


6.022x10²³ representative particles

b)


molar mass in grams

c)


22.4L of gas at STP

d)

All of these are correct

77.

if I initially have 4.0L of a gas and a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)


1.3 L

b)


13 L

c)


130 L

d)


400 L

78.

A substance that is dissolved by a solvent.

a)


Solvent

b)


Solute

c)


Solution

d)


Solvation

79.

The concentration determined by the moles of solute per liter of solution.

a)


%-Mass

b)


%-Volume

c)


Molarity

d)


Molality

80.

A substance that can donate hydrogen cations.

a)


Arrhenius Acid

b)


Arrhenius Base

c)


Bronsted-Lowry Acid

d)


Bronsted-Lowry Base

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