Question 1

Which term refers to a quantity of heat transferred at constant pressure?

Accepted Answer

A)  work 
B)  specific heat capacity 
C)  expansion 
D)  entropy 
E)  enthalpy 
A)  work 
B)  specific heat capacity 
C)  expansion 
D)  entropy 
E)  enthalpy

Question 2

A bomb calorimeter has a heat capacity of 675 J/°C and contains 925 g of water. If the combustion of 0.500 mole of a hydrocarbon increases the temperature of the calorimeter from 24.26°C to 53.88°C, determine the enthalpy change per mole of hydrocarbon. The specific heat of water = 4.184 J g-1 °C-1.

Accepted Answer

A)  -94.8 kJ 
B)  -135 kJ 
C)  -229 kJ 
D)  -269 kJ 
E)  -802 kJ 
A)  -94.8 kJ 
B)  -135 kJ 
C)  -229 kJ 
D)  -269 kJ 
E)  -802 kJ

Question 3

Heating a 25.0 g sample of each substance below with 375 J of energy will cause which substance to have the greatest increase in temperature?

Accepted Answer

A)  copper (specific heat = 0.385 J g-1 °C-1) 
B)  gold (specific heat = 0.128 J g-1 °C-1) 
C)  iron (specific heat = 0.451 J g-1 °C-1) 
D)  water (specific heat = 4.184 J g-1 °C-1) 
E)  Not enough information to determine. 
A)  copper (specific heat = 0.385 J g-1 °C-1) 
B)  gold (specific heat = 0.128 J g-1 °C-1) 
C)  iron (specific heat = 0.451 J g-1 °C-1) 
D)  water (specific heat = 4.184 J g-1 °C-1) 
E)  Not enough information to determine.

Question 4

How many kilojoules are there in 150 Calories of popcorn?

Accepted Answer

A)  3.6 × 10-2 kJ 
B)  36 kJ 
C)  630 kJ 
D)  3.6 × 104 kJ 
E)  6.3 × 105 kJ 
A)  3.6 × 10-2 kJ 
B)  36 kJ 
C)  630 kJ 
D)  3.6 × 104 kJ 
E)  6.3 × 105 kJ

Question 5

The standard enthalpies of formation for several substances are given below:   Determine the heat of vaporization for H2O and C2H5OH.

Accepted Answer

A)  241.8 and -235.1 kJ 
B)  241.8 and 325.1 kJ 
C)  44.0 and 42.6 kJ 
D)  -54.0 and -42.6 kJ 
E)  -44.0 and -42.6 kJ 
A)  241.8 and -235.1 kJ 
B)  241.8 and 325.1 kJ 
C)  44.0 and 42.6 kJ 
D)  -54.0 and -42.6 kJ 
E)  -44.0 and -42.6 kJ

Question 6

Determine the heat of reaction for the process  
using the information given below:

Accepted Answer

A)  -320.1 kJ 
B)  -233.7 kJ 
C)  233.7 kJ 
D)  320.1 kJ 
E)  504.7 kJ 
A)  -320.1 kJ 
B)  -233.7 kJ 
C)  233.7 kJ 
D)  320.1 kJ 
E)  504.7 kJ

Question 7

Determine if each of the four situations below describes kinetic or potential energy.
I. the bonds in propane molecules
II. a reservoir of water behind a dam
III. water molecules colliding into each other
IV. the electrical current in a light bulb that is turned on

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 8

According to the First Law of Thermodynamics, the total _____________ of the universe is constant.

Accepted Answer

The answer of According to the First Law of Thermodynamics,...

Question 9

Enthalpy change is equal to heat transfer at constant _______________.

Accepted Answer

The answer of Enthalpy change is equal to heat transfer...

Question 10

Determine the incorrect relationship given below.

Accepted Answer

A)  1 µJ = 1 × 10-6 J 
B)  1000 cal = 1 kcal 
C)  44.0 kJ = 1.05 × 104 cal 
D)  1000 J = 1 kJ 
E)  80.0 cal/g = 312 J/g 
A)  1 µJ = 1 × 10-6 J 
B)  1000 cal = 1 kcal 
C)  44.0 kJ = 1.05 × 104 cal 
D)  1000 J = 1 kJ 
E)  80.0 cal/g = 312 J/g

Question 11

Match between columns
                        Premises: energy of motion
chemical reaction that absorbs energy from surroundings
the energy of the universe is constant
energy required to raise 1 g of a substance 1°C
capacity to do work
heat transfer at constant pressure
used to calculate a standard enthalpy change
gravitational energy
chemical reaction that releases energy to the surroundings

Accepted Answer

The Answer of endothermic reaction and Hess' Law and potential is...

Question 12

Energy of motion is called _____________.

Accepted Answer

The answer of Energy of motion is called _____________....

Question 13

Which property can be used to distinguish one substance from another substance?

Accepted Answer

A)  specific heat capacity 
B)  kinetic energy 
C)  temperature 
D)  enthalpy 
E)  internal energy 
A)  specific heat capacity 
B)  kinetic energy 
C)  temperature 
D)  enthalpy 
E)  internal energy

Question 14

Heating a 50.0 g sample of iron (specific heat = 0.451 J g-1 °C-1) raises its temperature from 25.0°C to 79.4°C. How much energy was required to heat the sample?

Accepted Answer

A)  0.414 J 
B)  2.41 J 
C)  564 J 
D)  1230 J 
E)  1790 J 
A)  0.414 J 
B)  2.41 J 
C)  564 J 
D)  1230 J 
E)  1790 J

Question 15

What is the molar heat capacity of table salt, NaCl (specific heat = 0.88 J g-1 °C-1)?

Accepted Answer

A)  5.30 × 1022 J mol-1 °C-1 
B)  24.6 J mol-1 °C-1 
C)  51.4 J mol-1 °C-1 
D)  117 J mol-1 °C-1 
E)  245 J mol-1 °C-1 
A)  5.30 × 1022 J mol-1 °C-1 
B)  24.6 J mol-1 °C-1 
C)  51.4 J mol-1 °C-1 
D)  117 J mol-1 °C-1 
E)  245 J mol-1 °C-1

Which term refers to a quantity of heat transferred at constant pressure?

Heating a 25.0 g sample of each substance below with 375 J of energy will cause which substance to have the greatest increase in temperature?

How many kilojoules are there in 150 Calories of popcorn?

The standard enthalpies of formation for several substances are given below: Determine the heat of vaporization for H₂O and C₂H₅OH.

Determine the heat of reaction for the process using the information given below:

Determine if each of the four situations below describes kinetic or potential energy. I. the bonds in propane molecules II. a reservoir of water behind a dam III. water molecules colliding into each other IV. the electrical current in a light bulb that is turned on

According to the First Law of Thermodynamics, the total _____________ of the universe is constant.

Enthalpy change is equal to heat transfer at constant _______________.

Determine the incorrect relationship given below.

Energy of motion is called _____________.

Which property can be used to distinguish one substance from another substance?

Heating a 50.0 g sample of iron (specific heat = 0.451 J g^-1 °C^-1) raises its temperature from 25.0°C to 79.4°C. How much energy was required to heat the sample?

What is the molar heat capacity of table salt, NaCl (specific heat = 0.88 J g^-1 °C^-1)?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

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Exam 6: Energy and Chemical Reactions

Which term refers to a quantity of heat transferred at constant pressure?

Heating a 25.0 g sample of each substance below with 375 J of energy will cause which substance to have the greatest increase in temperature?

How many kilojoules are there in 150 Calories of popcorn?

The standard enthalpies of formation for several substances are given below: Determine the heat of vaporization for H2O and C2H5OH.

Determine the heat of reaction for the process using the information given below:

Determine if each of the four situations below describes kinetic or potential energy. I. the bonds in propane molecules II. a reservoir of water behind a dam III. water molecules colliding into each other IV. the electrical current in a light bulb that is turned on

According to the First Law of Thermodynamics, the total _____________ of the universe is constant.

Enthalpy change is equal to heat transfer at constant _______________.

Determine the incorrect relationship given below.

Energy of motion is called _____________.

Which property can be used to distinguish one substance from another substance?

Heating a 50.0 g sample of iron (specific heat = 0.451 J g-1 °C-1) raises its temperature from 25.0°C to 79.4°C. How much energy was required to heat the sample?

What is the molar heat capacity of table salt, NaCl (specific heat = 0.88 J g-1 °C-1)?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

Filters

The standard enthalpies of formation for several substances are given below: Determine the heat of vaporization for H₂O and C₂H₅OH.

Heating a 50.0 g sample of iron (specific heat = 0.451 J g^-1 °C^-1) raises its temperature from 25.0°C to 79.4°C. How much energy was required to heat the sample?

What is the molar heat capacity of table salt, NaCl (specific heat = 0.88 J g^-1 °C^-1)?