Use the following information to determine the enthalpy for the reaction shown below. CS2(l) F1F1F1S1F1F1F103O2(g) F1F1F1S1F1F1F10CO2(g) F1F1F1S1F1F1F102SO2(g) F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 ? C(graphite) F1F1F1S1F1F1F10O2(g) F1F1F1S1F1F1F10CO2(g) F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10393.5 kJ S(s) F1F1F1S1F1F1F10O2(g) F1F1F1S1F1F1F10SO2(g) F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10296.8 kJ C(graphite) F1F1F1S1F1F1F10 2S(s) F1F1F1S1F1F1F10CS2(l) F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 87.9 kJ

A) (F1F1F1S1F1F1F101075 kJ) B) (F1F1F1S1F1F1F101075 kJ) C) (F1F1F1S1F1F1F10778 kJ) D) (F1F1F1S1F1F1F10778 kJ) E) (F1F1F1S1F1F1F10602 kJ) A) (F1F1F1S1F1F1F101075 kJ) B) (F1F1F1S1F1F1F101075 kJ) C) (F1F1F1S1F1F1F10778 kJ) D) (F1F1F1S1F1F1F10778 kJ) E) (F1F1F1S1F1F1F10602 kJ)

Describe the difference between the change in the internal energy (F1F1F1S1F1F1F10E) of a system and the change in enthalpy (F1F1F1S1F1F1F10H). Begin your description with the definition of enthalpy change.

The enthalpy change is the energy that i

Given the following thermochemical equation detailing the combustion of methane CH4(g) F1F1F1S1F1F1F102O2(g) F1F1F1S1F1F1F10CO2(g) F1F1F1S1F1F1F102H2O(g) F1F1F1S1F1F1F10Hrxn F1F1F1S1F1F1F10 F1F1F1S1F1F1F10802kJ/mol CH4 Determine the amount of energy released when 25.0 g of methane undergoes combustion.

A) 1.95 F1F1F1S1F1F1F10 kJ B) 3.12 F1F1F1S1F1F1F10 kJ C) 453 kJ D) 1250 kJ E) 2.01 F1F1F1S1F1F1F10 kJ A) 1.95 F1F1F1S1F1F1F10 kJ B) 3.12 F1F1F1S1F1F1F10 kJ C) 453 kJ D) 1250 kJ E) 2.01 F1F1F1S1F1F1F10 kJ

Ethanol (CH3CH2OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is F1F1F1S1F1F1F10Hcomb F1F1F1S1F1F1F10 F1F1F1S1F1F1F101,368 kJ/mol, and its density is 0.789 g/mL. What is the fuel value of ethanol (kJ/g)?

A) 3.75 kJ/g B) 1,079 kJ/g C) 1,734 kJ/g D) 23.4 kJ/g E) 29.7 kJ/g A) 3.75 kJ/g B) 1,079 kJ/g C) 1,734 kJ/g D) 23.4 kJ/g E) 29.7 kJ/g

In an experiment, 5.0 g of ice at F1F1F1S1F1F1F1012 F1F1F1S1F1F1F10is converted into steam with a temperature of 120 F1F1F1S1F1F1F10. How much energy is required for this process?F1F1F1S1F1F1F10F1F1F1S1F1F1F10 F1F1F1S1F1F1F10F1F1F1S1F1F1F10vap F1F1F1S1F1F1F10 2,260 J/g; F1F1F1S1F1F1F10Hfus F1F1F1S1F1F1F10 334 J/g; cs(ice) F1F1F1S1F1F1F10 2.06 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10); cs(water) F1F1F1S1F1F1F10 4.18 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10); cs(steam) F1F1F1S1F1F1F10 1.99 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10))

A) 11.3 kJ B) 2.09 kJ C) 0.199 kJ D) 15.4 kJ E) 30.8 kJ A) 11.3 kJ B) 2.09 kJ C) 0.199 kJ D) 15.4 kJ E) 30.8 kJ

Exam 5: Thermochemistry: Energy Changes in Reactions

Use the following information to determine the enthalpy for the reaction shown below. CS₂(l) 3O₂(g) CO₂(g) 2SO₂(g) H  ? C(graphite) O₂(g) CO₂(g) H  393.5 kJ S(s) O₂(g) SO₂(g) H  296.8 kJ C(graphite)  2S(s) CS₂(l) H  87.9 kJ

(Multiple Choice)

4.9/5

(28)

Question 21

For which reaction below does the enthalpy change under standard conditions correspond to a standard enthalpy of formation?

(Multiple Choice)

4.8/5

(42)

Question 22

Benzoic acid is used to determine the heat capacity of bomb calorimeters because it can be obtained in pure form, and its energy of combustion is known very accurately (26.43 kJ/g). Determine the heat capacity of a calorimeter that had a temperature increase of 8.199C when 2.500 g of benzoic acid was used.

(Short Answer)

4.9/5

(34)

Question 23

Describe the difference between the change in the internal energy (E) of a system and the change in enthalpy (H). Begin your description with the definition of enthalpy change.

(Essay)

4.7/5

(29)

Question 24

Given the following thermochemical equation detailing the combustion of methane CH₄(g) 2O₂(g) CO₂(g) 2H₂O(g) H_rxn 802kJ/mol CH₄ Determine the amount of energy released when 25.0 g of methane undergoes combustion.

(Multiple Choice)

4.8/5

(35)

Question 25

The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO₂. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? ReactionH (kJ) SiO₂(s) 2C(s) Si(impure s) 2CO(g)690 Si(impure s) 2Cl₂(g) SiCl₄(g)657 SiCl₄(g) 2Mg(s) 2MgCl₂(s) Si(s)625

(Multiple Choice)

4.9/5

(34)

Question 26

Explain what is meant by the term state function, and give an example of something that is a state function and something that is not a state function.

(Essay)

4.8/5

(43)

Question 27

Isooctane is a good model compound for gasoline. When 1.14 g of isooctane (114 g/mol) reacts with excess oxygen in a constant pressure calorimeter, the temperature of the calorimeter increases by 10.0^oC. The heat capacity of the calorimeter is 5.46 kJ/^oC. Determine the molar enthalpy of combustion of isooctane.

(Multiple Choice)

4.8/5

(51)

Question 28

Ethanol (CH₃CH₂OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is H_comb  1,368 kJ/mol, and its density is 0.789 g/mL. What is the fuel value of ethanol (kJ/g)?

(Multiple Choice)

4.8/5

(45)

Question 29

According to Coulomb's law, which ionic compound A-D has the smallest electrostatic potential energy (i.e., closest to zero)? The size of the anion increases in the order F < Cl < Br < I.

(Multiple Choice)

4.7/5

(35)

Question 30

Which statement A-D about a state function is not correct?

(Multiple Choice)

4.7/5

(35)

Question 31

Which of the following objects will cool the fastest from the same initial temperature, assuming you had equal masses of each?

(Multiple Choice)

4.9/5

(29)

Question 32

In an experiment, 5.0 g of ice at 12 is converted into steam with a temperature of 120 . How much energy is required for this process? _vap  2,260 J/g; H_fus  334 J/g; c_s(ice)  2.06 J/(g  ); c_s(water)  4.18 J/(g  ); c_s(steam)  1.99 J/(g  ))

(Multiple Choice)

4.8/5

(33)

Question 33

Energy that an object has by virtue of its position is called ________

(Multiple Choice)

4.9/5

(41)

Question 34

What will be the final temperature of a 10.0 g piece of iron (C_P  25.09 J/(mol · )) initially at 25C, if it is supplied with 9.5 J from a stove?

(Multiple Choice)

4.8/5

(37)

Question 35

Which of the following bar charts shows the correct internal energy changes that occur when a propane grill is used to cook a steak? (Consider the propane combustion reaction to be the system. Consider the grill, steak, and everything else to be the surroundings.)

(Multiple Choice)

4.9/5

(30)

Question 36

Assuming that the distance between ions remains constant in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

(Multiple Choice)

4.8/5

(44)

Question 37

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents cooling of the gas?

(Multiple Choice)

4.8/5

(38)

Question 38

The diagram below shows three ion pairs: (a) a doubly charged anion and cation, (b) a singly charged anion and cation, and (c) two doubly charged anions. (I) Label each pair to identify the electrostatic interaction as attractive or as repulsive. (II) Which pair has the largest electrostatic interaction energy that is positive? (III) Which pair has the largest electrostatic interaction energy that is negative? (IV) Which pair has the smallest electrostatic interaction energy? (a) (b) (c)

(Essay)

4.9/5

(38)

Question 39

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents the liquid-to-solid transition?

(Multiple Choice)

4.9/5

(37)

Question 40

Showing 21 - 40 of 139

Use the following information to determine the enthalpy for the reaction shown below. CS₂(l) 3O₂(g) CO₂(g) 2SO₂(g) H  ? C(graphite) O₂(g) CO₂(g) H  393.5 kJ S(s) O₂(g) SO₂(g) H  296.8 kJ C(graphite)  2S(s) CS₂(l) H  87.9 kJ

For which reaction below does the enthalpy change under standard conditions correspond to a standard enthalpy of formation?

Describe the difference between the change in the internal energy (E) of a system and the change in enthalpy (H). Begin your description with the definition of enthalpy change.

Given the following thermochemical equation detailing the combustion of methane CH₄(g) 2O₂(g) CO₂(g) 2H₂O(g) H_rxn 802kJ/mol CH₄ Determine the amount of energy released when 25.0 g of methane undergoes combustion.

Explain what is meant by the term state function, and give an example of something that is a state function and something that is not a state function.

Ethanol (CH₃CH₂OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is H_comb  1,368 kJ/mol, and its density is 0.789 g/mL. What is the fuel value of ethanol (kJ/g)?

According to Coulomb's law, which ionic compound A-D has the smallest electrostatic potential energy (i.e., closest to zero)? The size of the anion increases in the order F < Cl < Br < I.

Which statement A-D about a state function is not correct?

Which of the following objects will cool the fastest from the same initial temperature, assuming you had equal masses of each?

In an experiment, 5.0 g of ice at 12 is converted into steam with a temperature of 120 . How much energy is required for this process? _vap  2,260 J/g; H_fus  334 J/g; c_s(ice)  2.06 J/(g  ); c_s(water)  4.18 J/(g  ); c_s(steam)  1.99 J/(g  ))

Energy that an object has by virtue of its position is called ________

What will be the final temperature of a 10.0 g piece of iron (C_P  25.09 J/(mol · )) initially at 25C, if it is supplied with 9.5 J from a stove?

Which of the following bar charts shows the correct internal energy changes that occur when a propane grill is used to cook a steak? (Consider the propane combustion reaction to be the system. Consider the grill, steak, and everything else to be the surroundings.)

Assuming that the distance between ions remains constant in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents cooling of the gas?

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents the liquid-to-solid transition?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 5: Thermochemistry: Energy Changes in Reactions

Use the following information to determine the enthalpy for the reaction shown below. CS2(l) 3O2(g) CO2(g) 2SO2(g) H  ? C(graphite) O2(g) CO2(g) H  393.5 kJ S(s) O2(g) SO2(g) H  296.8 kJ C(graphite)  2S(s) CS2(l) H  87.9 kJ

For which reaction below does the enthalpy change under standard conditions correspond to a standard enthalpy of formation?

Describe the difference between the change in the internal energy (E) of a system and the change in enthalpy (H). Begin your description with the definition of enthalpy change.

Given the following thermochemical equation detailing the combustion of methane CH4(g) 2O2(g) CO2(g) 2H2O(g) Hrxn  802kJ/mol CH4 Determine the amount of energy released when 25.0 g of methane undergoes combustion.

Explain what is meant by the term state function, and give an example of something that is a state function and something that is not a state function.

Ethanol (CH3CH2OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is Hcomb  1,368 kJ/mol, and its density is 0.789 g/mL. What is the fuel value of ethanol (kJ/g)?

According to Coulomb's law, which ionic compound A-D has the smallest electrostatic potential energy (i.e., closest to zero)? The size of the anion increases in the order F < Cl < Br < I.

Which statement A-D about a state function is not correct?

Which of the following objects will cool the fastest from the same initial temperature, assuming you had equal masses of each?

In an experiment, 5.0 g of ice at 12 is converted into steam with a temperature of 120 . How much energy is required for this process? vap  2,260 J/g; Hfus  334 J/g; cs(ice)  2.06 J/(g  ); cs(water)  4.18 J/(g  ); cs(steam)  1.99 J/(g  ))

Energy that an object has by virtue of its position is called ________

What will be the final temperature of a 10.0 g piece of iron (CP  25.09 J/(mol · )) initially at 25C, if it is supplied with 9.5 J from a stove?

Which of the following bar charts shows the correct internal energy changes that occur when a propane grill is used to cook a steak? (Consider the propane combustion reaction to be the system. Consider the grill, steak, and everything else to be the surroundings.)

Assuming that the distance between ions remains constant in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents cooling of the gas?

A cooling curve for some substance is shown below. Which of the line segments (I-V) represents the liquid-to-solid transition?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Use the following information to determine the enthalpy for the reaction shown below. CS₂(l) 3O₂(g) CO₂(g) 2SO₂(g) H  ? C(graphite) O₂(g) CO₂(g) H  393.5 kJ S(s) O₂(g) SO₂(g) H  296.8 kJ C(graphite)  2S(s) CS₂(l) H  87.9 kJ

Given the following thermochemical equation detailing the combustion of methane CH₄(g) 2O₂(g) CO₂(g) 2H₂O(g) H_rxn 802kJ/mol CH₄ Determine the amount of energy released when 25.0 g of methane undergoes combustion.

Ethanol (CH₃CH₂OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is H_comb  1,368 kJ/mol, and its density is 0.789 g/mL. What is the fuel value of ethanol (kJ/g)?

In an experiment, 5.0 g of ice at 12 is converted into steam with a temperature of 120 . How much energy is required for this process? _vap  2,260 J/g; H_fus  334 J/g; c_s(ice)  2.06 J/(g  ); c_s(water)  4.18 J/(g  ); c_s(steam)  1.99 J/(g  ))

What will be the final temperature of a 10.0 g piece of iron (C_P  25.09 J/(mol · )) initially at 25C, if it is supplied with 9.5 J from a stove?