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Chem Final

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Chemistry Final Part Two

Question 1 of 91

1

How many joules are there in 115 calories? (1cal = 4.18 J)

Select one of the following:

  • 2.9 J

  • 4.8 J

  • 28 J

  • 481 J

  • 11500 J

Explanation

Question 2 of 91

1

Which of the following has the greatest heat capacity?

Select one of the following:

  • 1000 g of water

  • 1000 g of steel

  • 1 g of water

  • 1 g of steel

Explanation

Question 3 of 91

1

Which of the following substances has the highest specific heat?

Select one of the following:

  • steel

  • water

  • alcohol

  • chloroform

Explanation

Question 4 of 91

1

What is the amount of heat required to raise the temperature of 100 g aluminum by 10 °C? (specific heat of aluminum = 0.21 cal/g x °C)

Select one of the following:

  • 0.21 cal

  • 2.1 cal

  • 210 cal

  • 21000 cal

  • None of the above

Explanation

Question 5 of 91

1

What is the specific heat of a substance if 1560 cal is required to raise the temperature of a 312-g sample by 15 °C?

Select one of the following:

  • 0.033 cal/g x °C

  • 0.33 cal/g x ºC

  • 0.99 cal/g x ºC

  • 1.33 cal/g x ºC

Explanation

Question 6 of 91

1

How many kilocalories of heat are required to raise the temperature of the 225 g of Al from 20 ºC to 100 ºC? (specific heat of aluminum = 0.21 cal/g x ºC)

Select one of the following:

  • 0.59 kcal

  • 3.8 kcal

  • 85 kcal

  • None of the above

Explanation

Question 7 of 91

1

The heat capacity of an object depends in part on its______.

Select one of the following:

  • mass

  • enthalpy

  • shape

  • potential energy

Explanation

Question 8 of 91

1

The amount of heat transferred from an object depend on all of the following except ______.

Select one of the following:

  • the specific heat of the object

  • the change in temperature the object undergoes

  • the initial temperature of the object

  • the mass of the object

Explanation

Question 9 of 91

1

A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?

Select one of the following:

  • The temperature of the metal will increase.

  • The temperature of the water will increase.

  • The temperature of the water will decrease.

  • The temperature of the water will increase and the temperature of the metal will decrease.

  • The temperature of the water will decrease and the temperature of the metal will increase.

Explanation

Question 10 of 91

1

Two objects are sitting next to each other in direct sunlight. Object A gets hotter than object B.

Select one of the following:

  • Object A has a higher specific heat than object B.

  • Object A has a lower specific heat than object B.

  • Both object have the same specific heat.

Explanation

Question 11 of 91

1

In an exothermic reaction, the energy stored in the chemical bonds of the reactants is ______.

Select one of the following:

  • equal to the energy stored in the bonds of the products

  • greater than the energy stored in the bonds of the products

  • less than the energy stored in the bonds of the products

  • less than the heat released

  • less than the heat absorbed

Explanation

Question 12 of 91

1

Compared to 100 g of iron, a 10-g sample of iron has ______.

Select one of the following:

  • a higher specific heat.

  • a lower specific heat.

  • the same specific heat.

Explanation

Question 13 of 91

1

If the heat involved in a chemical reaction has a negative sign, _____.

Select one of the following:

  • heat is lost to the surroundings

  • heat is gained from the surroundings

Explanation

Question 14 of 91

1

A process that absorbs heat is a(n) ______ process.

Select one of the following:

  • exothermic

  • endothermic

  • polythermic

  • ectothermic

Explanation

Question 15 of 91

1

If you were to touch the flask in which an endothermic reaction were occurring, _____.

Select one of the following:

  • the flask would probably feel cooler than before the reaction started

  • the flask would probably feel warmer than before the reaction started

  • the flask would feel the same as before the reaction started

  • None of the above

Explanation

Question 16 of 91

1

The amount of heat released by the complete burning of 1 mole of a substance is the _____.

Select one of the following:

  • specific heat

  • heat of combustion

  • heat capacity

  • system heat

Explanation

Question 17 of 91

1

The following equation shows the reaction that occurs when nitroglycerine explodes.
4 C3H5O9N3--> 12 CO2 + 10 6 N2 + O2 + 10 H2O + 1725 kcal
This reaction is ______.

Select one of the following:

  • endothermic

  • exothermic

  • a combination reaction

  • a combustion reaction

Explanation

Question 18 of 91

1

The amount of heat needed to melt one mole of a solid is called the _____.

Select one of the following:

  • molar heat of fusion

  • molar heat of solidification

  • heat of reaction

  • enthalpy

Explanation

Question 19 of 91

1

The amount of heat absorbed by a melting solid ______ the amount of heat lost by a solidifying liquid.

Select one of the following:

  • is the same as

  • is less than

  • is greater than

Explanation

Question 20 of 91

1

During a phase change, the temperature of a substance _____.

Select one of the following:

  • increases

  • decreases

  • remains constant

  • may increase or decrease

Explanation

Question 21 of 91

1

The vaporization of a liquid is an

Select one of the following:

  • exothermic process

  • endothermic process

Explanation

Question 22 of 91

1

Hess's Law _____.

Select one of the following:

  • makes it possible to calculate △H for complicated chemical reactions

  • states that when you reverse a chemical equation, you must change the sign of △H

  • determines the way a calorimeter works

  • describes the vaporization of solids

Explanation

Question 23 of 91

1

The amount of heat involved in the creation of 1 mole of substance from its element is called _____.

Select one of the following:

  • enthalpy

  • heat of reaction

  • standard heat of formation

  • heat of solidification

Explanation

Question 24 of 91

1

To calculate the amount of heat absorbed as a substance melts, which of the following information is not needed?

Select one of the following:

  • the mass of the substance

  • the specific heat of the substance

  • the change in temperature

  • the density of the smaple

Explanation

Question 25 of 91

1

As the temperature of a sample of matter is increased, what happens to the average kinetic energy of the particles in the sample?

Select one of the following:

  • It decreases.

  • It increases.

  • It does not change.

Explanation

Question 26 of 91

1

When 45 g of an alloy at 100ºC is dropped into 100.0 g of water at 25 ºC, the final temperature is 37ºC. What is the specific heat of the alloy?

Select one of the following:

  • 0.423

  • 1.77

  • 9.88

  • 48.8

Explanation

Question 27 of 91

1

How much heat does it take to make the water in a teakettle boil if the water starts at 22ºC?

Select one of the following:

  • 88 calories

  • 88 joules

  • 88 Calories

  • Not enough information given.

Explanation

Question 28 of 91

1

To determine the heat change for a reaction in an aqueous solution, _____.

Select one of the following:

  • you need to know the specific heat of the reactants

  • you can mix the reactants in a calorimeter and measure the temperature change

  • you need to know the mass of the reactants

  • you cannot determine the heat change for this type of reaction

Explanation

Question 29 of 91

1

Which of the following equations correctly represents an endothermic reaction?

Select one of the following:

  • A + B --> C + D + heat

  • A + B + heat --> C + D

Explanation

Question 30 of 91

1

The quantity of heat required to change the temperature of 1 g of a substance by 1 ºC is defined as _____.

Select one of the following:

  • a joule

  • specific heat capacity

  • a calorie

  • density

Explanation

Question 31 of 91

1

For a given substance, the molar heat of fusion _____ the molar heat of vaporization.

Select one of the following:

  • always equals

  • is less than

  • is greater than

Explanation

Question 32 of 91

1

For a given substance, the molar heat of vaporization ______ the molar heat of condensation.

Select one of the following:

  • always equal

  • is less than

  • is greater than

Explanation

Question 33 of 91

1

Heat of solution is ______.

Select one of the following:

  • the amount of heat required to change a solid into a liquid

  • the amount of heat absorbed or released when a solid dissolves

  • the amount of heat required to change a vapor into a liquid

  • the amount of heat released when a vapor changes into a liquid

Explanation

Question 34 of 91

1

The heat of formation for an element in its standard state is ______.

Select one of the following:

  • always zero

  • sometimes zero

  • never zero

Explanation

Question 35 of 91

1

When heat is added to boiling water, its temperature ______.

Select one of the following:

  • increases

  • decreases

  • stays the same

  • depends on the amount of water

Explanation

Question 36 of 91

1

Compared to a glass of ice water with ice in it, a glass of ice-cold water without ice will warm up _____.

Select one of the following:

  • faster

  • slower

  • at the same rate

Explanation

Question 37 of 91

1

When snow melts, what happens to the surrounding air?

Select one of the following:

  • It gets warmer.

  • It gets cooler.

  • Nothing happens to the surrounding air.

Explanation

Question 38 of 91

1

Why does air leave a tire when the tire valve is opened?

Select one of the following:

  • because the pressure outside the tire is lower than the pressure inside the tire

  • because the pressure outside the tire is greater than the pressure inside the tire

  • because the temperature is higher outside the tire than inside the tire

  • because there are more gas particles outside the tire than inside the tire

Explanation

Question 39 of 91

1

Which of these changes would NOT cause an increase in the the pressure of a gaseous system?

Select one of the following:

  • The container is made larger.

  • Additional amounts of the same gas are added to the container.

  • The temperature is increased.

  • Another gas is added to the container.

Explanation

Question 40 of 91

1

If the volume of a container holding gas is reduced, what will happen to the pressure within the containers?

Select one of the following:

  • The pressure will increase.

  • The pressure will not change.

  • The pressure will decrease.

Explanation

Question 41 of 91

1

What happens to the temperature of a gas when it is compressed?

Select one of the following:

  • The temperature increases.

  • The temperature does not change.

  • The temperature decreases.

Explanation

Question 42 of 91

1

Why does an aerosol can become cooler when gas is released?

Select one of the following:

  • because the propellant expands

  • because the propellant contracts

  • because the product expands with the can

  • because the volume of the can decreases

Explanation

Question 43 of 91

1

As the temperature of the gas in a balloon decreases _____.

Select one of the following:

  • the volume increases

  • the average kinetic energy of the gas decreases

  • the pressure increases

  • All of the above

Explanation

Question 44 of 91

1

If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen within the container?

Select one of the following:

  • It is reduced by one-half.

  • It is unchanged.

  • It is doubled.

Explanation

Question 45 of 91

1

Boyle's law states that _____.

Select one of the following:

  • the volume of a gas varies inversely with pressure

  • the volume of a gas varies directly with pressure

  • the temperature of a gas varies inversely with pressure

  • the temperature of a gas varies directly with pressure

Explanation

Question 46 of 91

1

When the temperature and number of particles are kept constant for a sample of gas, which of the following os also constant for the sample?

Select one of the following:

  • the sum of the pressure and volume

  • the difference of the pressure and volume

  • the product of the pressure and volume

  • the quotient of the pressure and volume

Explanation

Question 47 of 91

1

The volume of a gas is doubled while the temperature is held constant. The pressure of the gas _____.

Select one of the following:

  • is reduced by one-half

  • remains unchanged

  • is doubled

  • varies depending on the nature of the gas

Explanation

Question 48 of 91

1

The volume of a gas is reduced from 4L to 0.5 L while the temperature is held constant. The pressure of the gas ______.

Select one of the following:

  • increases by a factor of four

  • decreases by a factor of eight

  • increases by a factor of eight

  • increases by a factor of two

Explanation

Question 49 of 91

1

A gas occupies a volume of 0.2 L at 10.1 kPa. What volume will the gas occupy at 101 kPa?

Select one of the following:

  • 38 L

  • 20 L

  • 2 L

  • 0.02 L

Explanation

Question 50 of 91

1

Charles' Law states that _____.

Select one of the following:

  • the pressure of a gas is inversely proportional to its temperature in kelvins

  • the volume of a gas is directly proportional to its temperature in kelvins

  • the pressure of a gas is directly proportional to its temperature in kelvins

  • the volume of a gas is inversely proportional to its temperature in kelvins

Explanation

Question 51 of 91

1

A sample gas occupies 40.0 mL at -123 ºC. What volume does the sample occupy at 27 ºC?

Select one of the following:

  • 182 mL

  • 8.80 mL

  • 80.0 mL

  • 20.0 mL

Explanation

Question 52 of 91

1

If a balloon is rubbed vigorously, what happens to the pressure of the air inside the balloon if the volume remains constant?

Select one of the following:

  • It increases.

  • It stays the same.

  • It decreases.

Explanation

Question 53 of 91

1

When the volume and number of particles are held constant for a sample of gas, which of the following is also constant for the sample?

Select one of the following:

  • the sum of the pressure and temperature in kelvins

  • the difference of the pressure and temperature in kelvins

  • the product of the pressure and temperature in kelvins

  • the quotient of the pressure and temperature in kelvins

Explanation

Question 54 of 91

1

The combined gas law relates which of these?

Select one of the following:

  • pressure and volume only

  • temperature and pressure only

  • volume and temperature only

  • temperature, pressure, and volume

Explanation

Question 55 of 91

1

At a certain temperature and pressure, 0.20 mol of CO2 has a volume of 3.1 L. A 3.1-L sample of hydrogen at the same temperature and pressure ______.

Select one of the following:

  • has the same mass

  • contains the same number of atoms

  • has a higher density

  • contains the same number of molecules

Explanation

Question 56 of 91

1

Which of the following scientist developed an atomic theory in the early 1800s?

Select one of the following:

  • Isaac Newton

  • Antoine Lavoisier

  • Francis Bacon

  • Roger Bacon

  • John Dalton

Explanation

Question 57 of 91

1

Who discovered the electron?

Select one of the following:

  • Joseph Thomson

  • Niels Bohr

  • Ernest Rutherford

  • John Dalton

  • Albert Einstein

Explanation

Question 58 of 91

1

Which of the following is an accurate description of Thomson's model of the atom?

Select one of the following:

  • The electrons orbit the protons which are at the center of the atom

  • The electrons and protons move throughout the atom

  • Electrons occupy fixed positions around the protons, which are at the center of the atom

  • The electrons, like "raisins," are stuck into lump of protons, like "dough," in a "plum pudding" atom

Explanation

Question 59 of 91

1

In Rutherford's model of the atom, where are the electrons and protons located?

Select one of the following:

  • the electrons orbit the protons, which are at the center of the atom

  • the electrons and protons move throughout the atom

  • the electrons occupy fixed positions around the protons which are at the center of the atom

  • the electrons and protons are located throughout the atom, but they are not free to move

Explanation

Question 60 of 91

1

In Bohr's model of the atom, where are the electrons and protons located?

Select one of the following:

  • the electrons orbit the protons, which are at the center of the atom

  • the electrons and protons move throughout the atom

  • the electrons occupy fixed positions around the protons, which are at the center of the atom

  • the electrons and protons are located throughout the atom, but they are not free to move

Explanation

Question 61 of 91

1

In the Bohr model of the atom, an electron in an orbit has a fixed?

Select one of the following:

  • position

  • color

  • energy

Explanation

Question 62 of 91

1

What did Rutherford's experiment demonstrate?

Select one of the following:

  • that electrons orbit the nucleus

  • that all neutrons are located in the nucleus

  • that most of an atom's mass is concentrated in a relatively small portion of the atoms entire volume

  • that atoms are made of positively and negatively charged particles

Explanation

Question 63 of 91

1

Which of the following scientist developed the quantum mechanical model of the atom?

Select one of the following:

  • Albert Einstein

  • Erwin Schrsdinger

  • Niels Bohr

  • Ernest Rutherford

  • Joseph Tomson

Explanation

Question 64 of 91

1

What is the probability of finding an electron within the region indicated by the drawn electron cloud?

Select one of the following:

  • 50%

  • 67%

  • 75%

  • 90%

  • 100%

Explanation

Question 65 of 91

1

The quantum mechanical model of the atom _____.

Select one of the following:

  • defines the exact path of an electron around the nucleus

  • was proposed by Niels Bohr

  • is concerned with the probability of finding an election in a certain position

  • has many analogies in the visible world

Explanation

Question 66 of 91

1

The principal quantum number indicates what property of an electron

Select one of the following:

  • position

  • speed

  • energy level

  • electron cloud shape

  • spin

Explanation

Question 67 of 91

1

The shape (not the size) of an electron cloud is determined by the electrons

Select one of the following:

  • energy sublevel

  • spin

  • position

  • speed

  • principal quantum number

Explanation

Question 68 of 91

1

The 3p atomic orbital has the shape of ______.

Select one of the following:

  • a sphere

  • a dumbbell

  • a bar

  • two perpendicular dumbbells

  • an egg

Explanation

Question 69 of 91

1

How many energy sublevels are there in the second principal energy level?

Select one of the following:

  • 1

  • 2

  • 3

  • 4

  • 5

Explanation

Question 70 of 91

1

What types of atomic orbitals are in the third principal energy level?

Select one of the following:

  • s and p only

  • p and d only

  • s, p, and d only

  • p, d, and f only

Explanation

Question 71 of 91

1

How many f orbitals can there be in one atom?

Select one of the following:

  • 1

  • 3

  • 5

  • 7

  • 9

Explanation

Question 72 of 91

1

What is the maximum number of d orbitals in a principal energy level?

Select one of the following:

  • 1

  • 2

  • 3

  • 5

  • 10

Explanation

Question 73 of 91

1

What is the maximum number of orbitals in the p sub level?

Select one of the following:

  • 2

  • 3

  • 4

  • 5

  • 6

Explanation

Question 74 of 91

1

What is the maximum number of electrons in the second principal energy level?

Select one of the following:

  • 2

  • 8

  • 18

  • 32

Explanation

Question 75 of 91

1

Which of the following energy levels has the lowest energy?

Select one of the following:

  • 3d

  • 4s

  • 4p

  • 4f

Explanation

Question 76 of 91

1

If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?

Select one of the following:

  • zero

  • clockwise

  • counterclockwise

Explanation

Question 77 of 91

1

What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?

Select one of the following:

  • 2d

  • 2f

  • 3d

  • 3f

  • 4s

Explanation

Question 78 of 91

1

Which of the following states that no more than two electrons can occupy an atomic orbital and that two electrons in the same orbital must have opposite spins?

Select one of the following:

  • Hund's rule

  • Dalton's theory

  • the Aufbau principle

  • the Pauli exclusion principle

Explanation

Question 79 of 91

1

If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?

Select one of the following:

  • one electron in each orbital

  • two electrons in one orbital, one in another, none in the third

  • three in one orbital, none in the other two

Explanation

Question 80 of 91

1

What is the number of electrons in the outermost energy level of an oxygen atom?

Select one of the following:

  • 2

  • 4

  • 6

  • 8

  • 10

Explanation

Question 81 of 91

1

In order to occupy the same orbital, two electrons must have _____.

Select one of the following:

  • the same direction of spin

  • low energy

  • a high quantum number

  • opposite spin

Explanation

Question 82 of 91

1

According to the Aufbau principle _____.

Select one of the following:

  • an orbital may be occupied by only two electrons

  • electrons in the same orbital must have opposite spins

  • electrons enter orbitals of highest energy first

  • electrons enter orbitals of lowest energy first

Explanation

Question 83 of 91

1

What is the basis for exceptions to the Aufbau principle?

Select one of the following:

  • filled and half filled energy sub levels are more stable than partially-filled ones

  • electron configurations are only probable

  • electron spins are more important than energy levels in determining electron configuration

  • some elements have unusual atomic orbitals

Explanation

Question 84 of 91

1

Which of the following electromagnetic waves have the highest frequencies?

Select one of the following:

  • ultraviolet light waves

  • x-rays

  • microwaves

  • gamma rays

  • infrared light waves

Explanation

Question 85 of 91

1

Which color of visible light has the shortest wavelength?

Select one of the following:

  • orange

  • yellow

  • green

  • blue

  • violet

Explanation

Question 86 of 91

1

The quanta of light are called _____.

Select one of the following:

  • charms

  • excitons

  • muons

  • photons

  • solitons

Explanation

Question 87 of 91

1

The lowest energy state of an atom is called the _____.

Select one of the following:

  • excited state

  • ground state

  • independent state

  • dependent state

  • configurational state

Explanation

Question 88 of 91

1

To which variable of an object's wavelength directly proportional?

Select one of the following:

  • mass

  • velocity

  • temperature

  • position

  • None of the above

Explanation

Question 89 of 91

1

To which variable of an object is the object's mass directly proportional?

Select one of the following:

  • wavelength

  • velocity

  • temperature

  • position

  • frequency

Explanation

Question 90 of 91

1

Who developed the uncertainty principle?

Select one of the following:

  • Albert Einstein

  • Niels Bohr

  • Werner Heisenberg

  • Erwin Schrsdinger

  • Louis de Broglie

Explanation

Question 91 of 91

1

According to the uncertainty principle, if the position of a moving particle is known what other quantity cannot be known?

Select one of the following:

  • mass

  • temperature

  • charge

  • spin

  • velocity

Explanation

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