Using the following data for water, determine the final temperature when 100 g of ice at -10°C is heated with 350 kJ of energy. \[\begin{array} { | l | l | } \hline \text { Boiling point } & 373 \mathrm {~K} \\ \hline \text { Melting point } & 273 \mathrm {~K} \\ \hline \text { Enthalpy of vaporization } & 2,260 \mathrm {~J} / \mathrm { g } \\ \hline \text { Enthalpy of fusion } & 334 \mathrm {~J} / \mathrm { g } \\ \hline \text { Specific heat capacity (solid) } & 2.11 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\ \hline \text { Specific heat capacity (liquid) } & 4.18 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\ \hline \text { Specific heat capacity (gas) } & 2.08 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\ \hline \end{array}\]

A) 309°C B) 100°C C) 382°C D) 225°C E) 325°C A) 309°C B) 100°C C) 382°C D) 225°C E) 325°C

The enthalpy of combustion of table sugar (sucrose, C12H22O11, 342.3 g/mol) is -5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal = 4.184 kJ)

A) 3.94 Cal/g B) 11.1 Cal/g C) 16.5 Cal/g D) 2.92 Cal/g E) 1,350 Cal/g A) 3.94 Cal/g B) 11.1 Cal/g C) 16.5 Cal/g D) 2.92 Cal/g E) 1,350 Cal/g

Lightweight camping stoves typically use a mixture of C5 and C6 hydrocarbons, which is called white gas. Assuming white gas is 100% C5H12 with an enthalpy of combustion of -3,550 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20°C to 80°C? Assume all the energy is used to heat the water.

A) 8.96 g B) 7.64 g C) 9.65 g D) 6.99 g E) 10.73 g A) 8.96 g B) 7.64 g C) 9.65 g D) 6.99 g E) 10.73 g

Exam 5: Thermochemistry: Energy Changes in Reactions

Using the following data for water, determine the final temperature when 100 g of ice at -10°C is heated with 350 kJ of energy. Boiling point 373 Melting point 273 Enthalpy of vaporization 2,260/ Enthalpy of fusion 334/ Specific heat capacity (solid) 2.11/(\cdot) Specific heat capacity (liquid) 4.18/(\cdot) Specific heat capacity (gas) 2.08/(\cdot)

(Multiple Choice)

4.8/5

(33)

Question 21

The enthalpy of combustion of table sugar (sucrose, C₁₂H₂₂O₁₁, 342.3 g/mol) is -5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal = 4.184 kJ)

(Multiple Choice)

4.8/5

(31)

Question 22

Heat is best defined as ________

(Multiple Choice)

4.8/5

(36)

Question 23

In terms of the enthalpy of formation, which of the following compounds is the most unstable compared to its elements under standard conditions?

(Multiple Choice)

4.8/5

(38)

Question 24

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

(Multiple Choice)

4.9/5

(43)

Question 25

An expanding gas does 175 kJ of work on its surroundings at a constant pressure of 5.55 atm. If the gas initially occupied 125 mL, what is the final volume of the gas? (101.3 J = 1 L atm)

(Multiple Choice)

4.8/5

(45)

Question 26

You heat a cup of coffee in a microwave oven. It absorbs 40 kJ of energy from the microwave, and the volume expands. Which one of the following statements correctly describes the relationship between the change in enthalpy $\Delta$ H and the change in internal energy $\Delta$ E of the coffee? (> means greater than, < means less than)

(Multiple Choice)

4.9/5

(33)

Question 27

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?

(Essay)

4.9/5

(46)

Question 28

Thermochemistry is the study of how ________ is produced and consumed during chemical reactions.

(Multiple Choice)

4.9/5

(38)

Question 29

A balanced reaction equation with a $\Delta$ H value is called ________

(Multiple Choice)

4.8/5

(42)

Question 30

From year to year, the water level in a lake varies, as shown below. At which time is the potential energy of the water behind the dam greatest?

(Multiple Choice)

4.7/5

(34)

Question 31

Lightweight camping stoves typically use a mixture of C₅ and C₆ hydrocarbons, which is called white gas. Assuming white gas is 100% C₅H₁₂ with an enthalpy of combustion of -3,550 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20°C to 80°C? Assume all the energy is used to heat the water.

(Multiple Choice)

4.7/5

(44)

Question 32

When 1.14 g of octane (molar mass = 114 g/mol) reacts with excess oxygen in a constant volume calorimeter, the temperature of the calorimeter increases by 10.0°C. The heat capacity of the calorimeter is 6.97 kJ/°C. Determine the energy flow, q (reaction).

(Multiple Choice)

4.8/5

(45)

Question 33

When solid sodium hydroxide (NaOH) pellets are dissolved in water, the temperature of the water and beaker rises. This is an example of ________

(Multiple Choice)

4.8/5

(37)

Question 34

Which statement A-D about the first law of thermodynamics ( $\Delta$ E_system= q + w) is not correct?

(Multiple Choice)

4.7/5

(38)

Question 35

During a(n) ________ process, energy is transferred from the system to the surroundings.

(Multiple Choice)

4.7/5

(42)

Question 36

Which of the following hydrocarbons has the greatest fuel value?

(Multiple Choice)

4.8/5

(42)

Question 37

You hold a 50 g sphere of copper in one hand and a 25 g sphere of aluminum in the other hand. If both absorb energy at the same rate, which will come to your body temperature first and why? The specific heat capacities are 0.4 J/(g .°C) for copper and 0.9 J/(g .°C) for aluminum.

(Multiple Choice)

4.8/5

(28)

Question 38

If a chemical reaction causes the temperature of the container to drop, it is a(n) ________ reaction.

(Multiple Choice)

4.7/5

(39)

Question 39

Which statement below regarding the various heat capacities is not correct?

(Multiple Choice)

4.8/5

(39)

Question 40

Showing 21 - 40 of 132

The enthalpy of combustion of table sugar (sucrose, C₁₂H₂₂O₁₁, 342.3 g/mol) is -5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal = 4.184 kJ)

Heat is best defined as ________

In terms of the enthalpy of formation, which of the following compounds is the most unstable compared to its elements under standard conditions?

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

An expanding gas does 175 kJ of work on its surroundings at a constant pressure of 5.55 atm. If the gas initially occupied 125 mL, what is the final volume of the gas? (101.3 J = 1 L atm)

Thermochemistry is the study of how ________ is produced and consumed during chemical reactions.

A balanced reaction equation with a $\Delta$ H value is called ________

From year to year, the water level in a lake varies, as shown below. At which time is the potential energy of the water behind the dam greatest?

When 1.14 g of octane (molar mass = 114 g/mol) reacts with excess oxygen in a constant volume calorimeter, the temperature of the calorimeter increases by 10.0°C. The heat capacity of the calorimeter is 6.97 kJ/°C. Determine the energy flow, q (reaction).

When solid sodium hydroxide (NaOH) pellets are dissolved in water, the temperature of the water and beaker rises. This is an example of ________

Which statement A-D about the first law of thermodynamics ( $\Delta$ E_system= q + w) is not correct?

During a(n) ________ process, energy is transferred from the system to the surroundings.

Which of the following hydrocarbons has the greatest fuel value?

You hold a 50 g sphere of copper in one hand and a 25 g sphere of aluminum in the other hand. If both absorb energy at the same rate, which will come to your body temperature first and why? The specific heat capacities are 0.4 J/(g .°C) for copper and 0.9 J/(g .°C) for aluminum.

If a chemical reaction causes the temperature of the container to drop, it is a(n) ________ reaction.

Which statement below regarding the various heat capacities is not correct?

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: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

Exam 5: Thermochemistry: Energy Changes in Reactions

The enthalpy of combustion of table sugar (sucrose, C12H22O11, 342.3 g/mol) is -5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal = 4.184 kJ)

Heat is best defined as ________

In terms of the enthalpy of formation, which of the following compounds is the most unstable compared to its elements under standard conditions?

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

An expanding gas does 175 kJ of work on its surroundings at a constant pressure of 5.55 atm. If the gas initially occupied 125 mL, what is the final volume of the gas? (101.3 J = 1 L atm)

Thermochemistry is the study of how ________ is produced and consumed during chemical reactions.

A balanced reaction equation with a Δ\DeltaΔ H value is called ________

From year to year, the water level in a lake varies, as shown below. At which time is the potential energy of the water behind the dam greatest?

When 1.14 g of octane (molar mass = 114 g/mol) reacts with excess oxygen in a constant volume calorimeter, the temperature of the calorimeter increases by 10.0°C. The heat capacity of the calorimeter is 6.97 kJ/°C. Determine the energy flow, q (reaction).

When solid sodium hydroxide (NaOH) pellets are dissolved in water, the temperature of the water and beaker rises. This is an example of ________

Which statement A-D about the first law of thermodynamics ( Δ\DeltaΔ Esystem = q + w) is not correct?

During a(n) ________ process, energy is transferred from the system to the surroundings.

Which of the following hydrocarbons has the greatest fuel value?

You hold a 50 g sphere of copper in one hand and a 25 g sphere of aluminum in the other hand. If both absorb energy at the same rate, which will come to your body temperature first and why? The specific heat capacities are 0.4 J/(g .°C) for copper and 0.9 J/(g .°C) for aluminum.

If a chemical reaction causes the temperature of the container to drop, it is a(n) ________ reaction.

Which statement below regarding the various heat capacities is not correct?

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: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

The enthalpy of combustion of table sugar (sucrose, C₁₂H₂₂O₁₁, 342.3 g/mol) is -5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal = 4.184 kJ)

A balanced reaction equation with a $\Delta$ H value is called ________

Which statement A-D about the first law of thermodynamics ( $\Delta$ E_system= q + w) is not correct?