Question 1

Which of the following statements concerning the physical states of the elements at room temperature (25º C) and pressure is incorrect?

Accepted Answer

A)  Only two elements, bromine and mercury, are liquids. 
B)  The vast majority of the elements are solids. 
C)  The gaseous state is more common than the liquid state. 
D)  Over half of all the elements are liquids. 
A)  Only two elements, bromine and mercury, are liquids. 
B)  The vast majority of the elements are solids. 
C)  The gaseous state is more common than the liquid state. 
D)  Over half of all the elements are liquids.

Question 2

How many Joules of heat must be removed to lower the temperature of a 36.5 g Al bar from 84.1 °C to 56.8 °C? The specific heat of Al is 0.908 J/g °C.

Accepted Answer

A)  581 J 
B)  1090 J 
C)  905 J 
D)  240 J 
A)  581 J 
B)  1090 J 
C)  905 J 
D)  240 J

Question 3

The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: CH4, CS2, KBr, NH3.

Accepted Answer

A)  CS2 4 3 
B)  CH4 2 3 3 2 4 
D)  CH4 3 2 
A)  CS2 4 3 
B)  CH4 2 3 3 2 4 
D)  CH4 3 2

Question 4

What is the heat capacity of 84.0 g of water? Specific heat of water = 4.18 J/(g °C)

Accepted Answer

A)  351 J/°C 
B)  96.8 J/°C 
C)  506 J/°C 
D)  492 J/°C 
A)  351 J/°C 
B)  96.8 J/°C 
C)  506 J/°C 
D)  492 J/°C

Question 5

If liquid methyl amine and hydrofluoric acid were mixed, between which two atoms in these molecules would a hydrogen bond form?

Accepted Answer

A)  between 4 and 5, between 2 and 5, or between 3 and 6 
B)  between 2 and 5 only 
C)  between 3 and 6 only 
D)  between 4 and 5 or 2 and 5 
A)  between 4 and 5, between 2 and 5, or between 3 and 6 
B)  between 2 and 5 only 
C)  between 3 and 6 only 
D)  between 4 and 5 or 2 and 5

Question 6

The anomalously high boiling point of water is due to ________.

Accepted Answer

A)  London forces 
B)  its low heat of vaporization 
C)  hydrogen bonding 
D)  ice being less dense than liquid water 
A)  London forces 
B)  its low heat of vaporization 
C)  hydrogen bonding 
D)  ice being less dense than liquid water

Question 7

A chocolate, caramel pecan piece of candy contains 115 food Calories (Cal). A food Calorie is equivalent to 1000 calories of heat energy. If the heat energy contained in the piece of candy were transferred to 53.5 kg of water at 25.0 °C, what would be the final temperature of the water? The specific heat of water is 4.18 J/g °C.

Accepted Answer

115 Cal × @#IMG-DLM& × @#IMG-DLM& = 4.8070 × 10⁵ J (calc) = 4

Question 8

Which of the following molecules are capable of hydrogen bonding with water?
H2S NH3 H2 HBr CH

Accepted Answer

A)  NH3, HBr, and H2 
B)  NH3 and HF 
C)  H2S and CH4 
D)  H2S, HBr, and H2 
A)  NH3, HBr, and H2 
B)  NH3 and HF 
C)  H2S and CH4 
D)  H2S, HBr, and H2

Question 9

Which of the following is not a correct characterization of the liquid state?

Accepted Answer

A)  The particles move relatively long distances before colliding with adjacent particles. 
B)  The particles are randomly packed in relatively close proximity to each other. 
C)  The particles "slide" freely over each other. 
D)  The particles do not have sufficient energy to separate from each other. 
A)  The particles move relatively long distances before colliding with adjacent particles. 
B)  The particles are randomly packed in relatively close proximity to each other. 
C)  The particles "slide" freely over each other. 
D)  The particles do not have sufficient energy to separate from each other.

Question 10

What would be the temperature change, in C, if 555 J of heat energy is added to 35.0 g of a metal with a specific heat of 0.418 J/g °C?

Accepted Answer

The answer of What would be the temperature change, in...

Question 11

The calculation below is set up to determine how much heat is needed to convert 50 g of ice at ?20 °C to steam at 300 °C. Which constant does A represent? (A)(50 g)(20 °C) + (heat of fusion)(50 g) + (4.18 J/g°C)(50 g)(100 °C) + (B)(50 g) + (C)(50 g )(200 °C) = total heat

Accepted Answer

A)  heat of condensation 
B)  specific heat of ice 
C)  specific heat of water 
D)  heat of vaporization of water 
A)  heat of condensation 
B)  specific heat of ice 
C)  specific heat of water 
D)  heat of vaporization of water

Question 12

Which one of the following is classified as a covalent solid?

Accepted Answer

A)  K2SO4 
B)  Cr 
C)  CO2 
D)  C 
A)  K2SO4 
B)  Cr 
C)  CO2 
D)  C

Question 13

The combustion of one mole of a gas produces 212 calories of energy. Express the energy released in this reaction in kilojoules.

Accepted Answer

A)  239 kJ 
B)  886 kJ 
C)  0.886 kJ 
D)  0.239 kJ 
A)  239 kJ 
B)  886 kJ 
C)  0.886 kJ 
D)  0.239 kJ

Question 14

According to kinetic molecular theory, the molecules of a gas ________.

Accepted Answer

A)  are constantly moving in a regular pattern 
B)  are constantly moving in a random manner 
C)  cannot move because of lack of space 
D)  move only at high temperatures (above 1000 
A)  are constantly moving in a regular pattern 
B)  are constantly moving in a random manner 
C)  cannot move because of lack of space 
D)  move only at high temperatures (above 1000

Question 15

A T-bone steak provides 6.90 x 102 food Calories (Cal). A food Calorie is equivalent to 4180 J of heat energy. The heat energy provided by the steak would be sufficient to heat 59.1 kg of water how many Celsius degrees. The specific heat of water is 4.18 J/g °C.

Accepted Answer

A)  6.58 °C 
B)  11.7 °C 
C)  9.20 °C 
D)  23.6 C 
A)  6.58 °C 
B)  11.7 °C 
C)  9.20 °C 
D)  23.6 C

Question 16

Which best describes the size and shape of a sample of liquid?

Accepted Answer

A)  definite volume and definite shape 
B)  volume and shape both determined by the container 
C)  definite volume, but shape is determined by the container 
D)  volume determined by container, but definite shape 
A)  definite volume and definite shape 
B)  volume and shape both determined by the container 
C)  definite volume, but shape is determined by the container 
D)  volume determined by container, but definite shape

Question 17

On the basis of your understanding of bonding in liquids and solids, arrange the following substances from the highest to lowest melting points: NaCl &ensp; Na &ensp; Cl2 &ensp; SiO2

Accepted Answer

A)  Cl2, Na, NaCl, SiO2 
B)  Na, NaCl, Cl2, SiO2 
C)  SiO2, NaCl, Na, Cl2 
D)  NaCl, SiO2, Na, Cl2 
A)  Cl2, Na, NaCl, SiO2 
B)  Na, NaCl, Cl2, SiO2 
C)  SiO2, NaCl, Na, Cl2 
D)  NaCl, SiO2, Na, Cl2

Question 18

The strength of London dispersion forces depends on what two factors?

Accepted Answer

A)  molecular mass and polarizability 
B)  vapor pressure and size 
C)  molecular mass and volatility 
D)  volatility and shape 
A)  molecular mass and polarizability 
B)  vapor pressure and size 
C)  molecular mass and volatility 
D)  volatility and shape

Question 19

The specific heat of substance A is one fourth that of substance B. The temperature of both a 24.0 g sample of substance A and a 12.0 g sample of substance B was raised 20 °C. The heat absorbed by substance A was ________ the heat absorbed by substance B.

Accepted Answer

A)  equal to 
B)  one-half 
C)  twice 
D)  four times 
A)  equal to 
B)  one-half 
C)  twice 
D)  four times

Question 20

Which of the following statements concerning temperature change as a substance is heated is incorrect?

Accepted Answer

A)  As a solid is heated, its temperature rises until its melting point is reached. 
B)  During the time a solid melts to a liquid the temperature remains constant. 
C)  As a liquid is heated, its temperature rises until its boiling point is reached. 
D)  During the time a liquid is changing to the gaseous state the temperature gradually increases while all the liquid is changed. 
A)  As a solid is heated, its temperature rises until its melting point is reached. 
B)  During the time a solid melts to a liquid the temperature remains constant. 
C)  As a liquid is heated, its temperature rises until its boiling point is reached. 
D)  During the time a liquid is changing to the gaseous state the temperature gradually increases while all the liquid is changed.

Which of the following statements concerning the physical states of the elements at room temperature (25º C) and pressure is incorrect?

How many Joules of heat must be removed to lower the temperature of a 36.5 g Al bar from 84.1 °C to 56.8 °C? The specific heat of Al is 0.908 J/g °C.

The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: CH₄, CS₂, KBr, NH₃.

What is the heat capacity of 84.0 g of water? Specific heat of water = 4.18 J/(g °C)

If liquid methyl amine and hydrofluoric acid were mixed, between which two atoms in these molecules would a hydrogen bond form?

The anomalously high boiling point of water is due to ________.

Which of the following molecules are capable of hydrogen bonding with water? H₂S NH₃ H₂ HBr CH

Which of the following is not a correct characterization of the liquid state?

What would be the temperature change, in C, if 555 J of heat energy is added to 35.0 g of a metal with a specific heat of 0.418 J/g °C?

The calculation below is set up to determine how much heat is needed to convert 50 g of ice at ?20 °C to steam at 300 °C. Which constant does A represent? (A)(50 g)(20 °C) + (heat of fusion)(50 g) + (4.18 J/g°C)(50 g)(100 °C) + (B)(50 g) + (C)(50 g )(200 °C) = total heat

Which one of the following is classified as a covalent solid?

The combustion of one mole of a gas produces 212 calories of energy. Express the energy released in this reaction in kilojoules.

According to kinetic molecular theory, the molecules of a gas ________.

A T-bone steak provides 6.90 x 10² food Calories (Cal). A food Calorie is equivalent to 4180 J of heat energy. The heat energy provided by the steak would be sufficient to heat 59.1 kg of water how many Celsius degrees. The specific heat of water is 4.18 J/g °C.

Which best describes the size and shape of a sample of liquid?

On the basis of your understanding of bonding in liquids and solids, arrange the following substances from the highest to lowest melting points: NaCl Na Cl₂ SiO₂

The strength of London dispersion forces depends on what two factors?

The specific heat of substance A is one fourth that of substance B. The temperature of both a 24.0 g sample of substance A and a 12.0 g sample of substance B was raised 20 °C. The heat absorbed by substance A was ________ the heat absorbed by substance B.

Which of the following statements concerning temperature change as a substance is heated is incorrect?

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Exam 11: States of Matter

Which of the following statements concerning the physical states of the elements at room temperature (25º C) and pressure is incorrect?

How many Joules of heat must be removed to lower the temperature of a 36.5 g Al bar from 84.1 °C to 56.8 °C? The specific heat of Al is 0.908 J/g °C.

The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: CH4, CS2, KBr, NH3.

What is the heat capacity of 84.0 g of water? Specific heat of water = 4.18 J/(g °C)

If liquid methyl amine and hydrofluoric acid were mixed, between which two atoms in these molecules would a hydrogen bond form?

The anomalously high boiling point of water is due to ________.

Which of the following molecules are capable of hydrogen bonding with water? H2S NH3 H2 HBr CH

Which of the following is not a correct characterization of the liquid state?

What would be the temperature change, in C, if 555 J of heat energy is added to 35.0 g of a metal with a specific heat of 0.418 J/g °C?

The calculation below is set up to determine how much heat is needed to convert 50 g of ice at ?20 °C to steam at 300 °C. Which constant does A represent? (A)(50 g)(20 °C) + (heat of fusion)(50 g) + (4.18 J/g°C)(50 g)(100 °C) + (B)(50 g) + (C)(50 g )(200 °C) = total heat

Which one of the following is classified as a covalent solid?

The combustion of one mole of a gas produces 212 calories of energy. Express the energy released in this reaction in kilojoules.

According to kinetic molecular theory, the molecules of a gas ________.

A T-bone steak provides 6.90 x 102 food Calories (Cal). A food Calorie is equivalent to 4180 J of heat energy. The heat energy provided by the steak would be sufficient to heat 59.1 kg of water how many Celsius degrees. The specific heat of water is 4.18 J/g °C.

Which best describes the size and shape of a sample of liquid?

On the basis of your understanding of bonding in liquids and solids, arrange the following substances from the highest to lowest melting points: NaCl Na Cl2 SiO2

The strength of London dispersion forces depends on what two factors?

The specific heat of substance A is one fourth that of substance B. The temperature of both a 24.0 g sample of substance A and a 12.0 g sample of substance B was raised 20 °C. The heat absorbed by substance A was ________ the heat absorbed by substance B.

Which of the following statements concerning temperature change as a substance is heated is incorrect?

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

Gas Laws

Solutions

Acids, Bases and Salts

Oxidation and Reduction

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: CH₄, CS₂, KBr, NH₃.

Which of the following molecules are capable of hydrogen bonding with water? H₂S NH₃ H₂ HBr CH

A T-bone steak provides 6.90 x 10² food Calories (Cal). A food Calorie is equivalent to 4180 J of heat energy. The heat energy provided by the steak would be sufficient to heat 59.1 kg of water how many Celsius degrees. The specific heat of water is 4.18 J/g °C.

On the basis of your understanding of bonding in liquids and solids, arrange the following substances from the highest to lowest melting points: NaCl Na Cl₂ SiO₂