What is the enthalpy change when 175 g of C3H8 are burned in excess O2?

A) -1.71 × 107 kJ B) -1.79 × 10-3 kJ C) -3.47 × 100 kJ D) -3.89 × 105 kJ E) -8.82 × 103 kJ A) -1.71 × 107 kJ B) -1.79 × 10-3 kJ C) -3.47 × 100 kJ D) -3.89 × 105 kJ E) -8.82 × 103 kJ

Exam 6: Energy and Chemical Reactions

A 0.100 mole sample of CH₄ reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g^-1 °C^-1.

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Question 1

Correct Answer:

Verified

The quantity of energy required to increase the temperature of one gram of a sample by 1°C is called the _____________.

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Question 2

Correct Answer:

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specific heat

Which of the following is an example of potential energy?

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Question 3

Correct Answer:

Verified

The temperature of a 21.6 g sample of a metal rises 6.04°C when 58.8 J of energy is applied to it. What is the identity of the metal?

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Question 4

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

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Question 5

What is the enthalpy change when 175 g of C₃H₈ are burned in excess O₂?

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Question 6

In a(n) _____________ reaction, the energy of bond breaking is greater than the energy of bond making.

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Question 7

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g^-1 °C^-1).

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Question 8

The First Law of Thermodynamics states that:

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Question 9

Which of the following is not an example of kinetic energy?

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Question 10

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

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Question 11

In an endothermic reaction, heat is transferred from the _ to the _.

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Question 12

Which substance has the highest molar heat capacity?

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Question 13

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g^-1 at 0 °C; the specific heat of water = 4.184 J g^-1 °C^-1; the heat of vaporization of water = 2260 J g^-1 at 100 °C.

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Question 14

A 20.0 g sample of aluminum (specific heat = 0.902 J g^-1 °C^-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

(Multiple Choice)

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Question 15

Which statement about energy is false?

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Question 16

Based on the following thermochemical equation, which statement is false?

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Question 17

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g^-1 °C^-1).

(Multiple Choice)

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Question 18

The complete combustion of 1.47 g of methanol produces 29.3 kJ of heat. Determine the DH° for the reaction and its sign.

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Question 19

Based on the following thermochemical equation below, which statement is false?

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Question 20

Showing 1 - 20 of 55

A 0.100 mole sample of CH₄ reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g^-1 °C^-1.

The quantity of energy required to increase the temperature of one gram of a sample by 1°C is called the _____________.

Which of the following is an example of potential energy?

The temperature of a 21.6 g sample of a metal rises 6.04°C when 58.8 J of energy is applied to it. What is the identity of the metal?

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

What is the enthalpy change when 175 g of C₃H₈ are burned in excess O₂?

In a(n) _____________ reaction, the energy of bond breaking is greater than the energy of bond making.

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g^-1 °C^-1).

The First Law of Thermodynamics states that:

Which of the following is not an example of kinetic energy?

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

In an endothermic reaction, heat is transferred from the _ to the _.

Which substance has the highest molar heat capacity?

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g^-1 at 0 °C; the specific heat of water = 4.184 J g^-1 °C^-1; the heat of vaporization of water = 2260 J g^-1 at 100 °C.

A 20.0 g sample of aluminum (specific heat = 0.902 J g^-1 °C^-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Which statement about energy is false?

Based on the following thermochemical equation, which statement is false?

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g^-1 °C^-1).

The complete combustion of 1.47 g of methanol produces 29.3 kJ of heat. Determine the DH° for the reaction and its sign.

Based on the following thermochemical equation below, which statement is false?

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Covalent Bonding

Molecular Structure

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Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

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Exam 6: Energy and Chemical Reactions

A 0.100 mole sample of CH4 reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g-1 °C-1.

The quantity of energy required to increase the temperature of one gram of a sample by 1°C is called the _____________.

Which of the following is an example of potential energy?

The temperature of a 21.6 g sample of a metal rises 6.04°C when 58.8 J of energy is applied to it. What is the identity of the metal?

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

What is the enthalpy change when 175 g of C3H8 are burned in excess O2?

In a(n) _____________ reaction, the energy of bond breaking is greater than the energy of bond making.

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g-1 °C-1).

The First Law of Thermodynamics states that:

Which of the following is not an example of kinetic energy?

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

In an endothermic reaction, heat is transferred from the _____________ to the _____________.

Which substance has the highest molar heat capacity?

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g-1 at 0 °C; the specific heat of water = 4.184 J g-1 °C-1; the heat of vaporization of water = 2260 J g-1 at 100 °C.

A 20.0 g sample of aluminum (specific heat = 0.902 J g-1 °C-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Which statement about energy is false?

Based on the following thermochemical equation, which statement is false?

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g-1 °C-1).

The complete combustion of 1.47 g of methanol produces 29.3 kJ of heat. Determine the DH° for the reaction and its sign.

Based on the following thermochemical equation below, which statement is false?

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

A 0.100 mole sample of CH₄ reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g^-1 °C^-1.

What is the enthalpy change when 175 g of C₃H₈ are burned in excess O₂?

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g^-1 °C^-1).

In an endothermic reaction, heat is transferred from the _ to the _.

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g^-1 at 0 °C; the specific heat of water = 4.184 J g^-1 °C^-1; the heat of vaporization of water = 2260 J g^-1 at 100 °C.

A 20.0 g sample of aluminum (specific heat = 0.902 J g^-1 °C^-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g^-1 °C^-1).