This Chemistry Ch16&17 Exam assesses knowledge in thermodynamics, focusing on concepts like enthalpy, entropy, and free energy changes. It includes practical energy conversion calculations and requires understanding of thermochemical equations and phase changes.
Thermochemical equation
Enthalpy of combustion
Molar enthalpy of vaporization
Molar enthalpy of fusion
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Thermochemical equation
Enthalpy of combustion
Molar enthalpy of vaporization
Molar enthalpy of fusion
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Thermochemical equation
Enthalpy of combustion
Molar enthalpy of vaporization
Molar enthalpy of fusion
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Thermochemical equation
Enthalpy of combustion
Molar enthalpy of vaporization
Molar enthalpy of fusion
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Thermochemical equation
Enthalpy of combustion
Molar enthalpy of vaporization
Molar enthalpy of fusion
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Cool
Released
Absorbs
Heat
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Cool
Released
Absorbs
Heat
Cool
Released
Absorbs
Heat
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Cool
Released
Absorbs
Heat
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Cool
Released
Absorbs
Heat
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Spontaneous process
Law of disorder
Entropy
Free energy
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Spontaneous process
Law of disorder
Entropy
Free energy
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Spontaneous process
Law of disorder
Entropy
Free energy
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Potential / kinetic
Exothermic / endothermic
Chemical
Universe
Standard
Same
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Potential / kinetic
Exothermic / endothermic
Chemical
Universe
Standard
Same
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Potential / kinetic
Exothermic / endothermic
Chemical
Universe
Standard
Same
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Potential / kinetic
Exothermic / endothermic
Chemical
Universe
Standard
Same
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Potential / kinetic
Exothermic / endothermic
Chemical
Universe
Standard
Same
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Calorimeter
Thermochemistry
System
Enthalpy (heat) of reaction
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Calorimeter
Thermochemistry
System
Enthalpy (heat) of reaction
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Calorimeter
Thermochemistry
System
Enthalpy (heat) of reaction
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Calorimeter
Thermochemistry
System
Enthalpy (heat) of reaction
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Universe
Enthalpy
Surroundings
Enthalpy (heat) of reaction
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Universe
Enthalpy
Surroundings
Enthalpy (heat) of reaction
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Universe
Enthalpy
Surroundings
Enthalpy (heat) of reaction
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Energy
Law of conservation of energy
Heat
Thermochemistry
Chemical potential energy
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Specific heat
Calorimeter
Universe
Law of disorder
Surroundings
Law of conservation of energy
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Energy
Law of conservation of energy
Heat
Thermochemistry
Chemical potential energy
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Energy
Law of conservation of energy
Heat
Thermochemistry
Chemical potential energy
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Energy
Law of conservation of energy
Heat
Thermochemistry
Chemical potential energy
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Energy
Law of conservation of energy
Heat
Thermochemistry
Chemical potential energy
Specific heat
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Enthalpy (heat) of reaction
Thermochemical equation
Universe
Enthalpy
Molar enthalpy (heat) of vaporization
Calorimeter
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Specific heat
Calorimeter
Universe
Law of disorder
Surroundings
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Specific heat
Calorimeter
Universe
Law of disorder
Surroundings
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Specific heat
Calorimeter
Universe
Law of disorder
Surroundings
Enthalpy (heat) of reaction
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Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
Thermochemical equation
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Enthalpy (heat) of reaction
Thermochemical equation
Universe
Enthalpy
Molar enthalpy (heat) of vaporization
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Enthalpy (heat) of reaction
Thermochemical equation
Universe
Enthalpy
Molar enthalpy (heat) of vaporization
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Enthalpy (heat) of reaction
Thermochemical equation
Universe
Enthalpy
Molar enthalpy (heat) of vaporization
Standard enthalpy (heat) of formation
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Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
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Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
Rate this question:
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
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Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
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Standard enthalpy (heat) of formation
Molar enthalpy (heat) of fusion
Spontaneous process
Enthalpy (heat) of combustion
Free energy
Joule
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Complex reaction
Elementary step
Reaction mechanism
Reaction order
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Zero
One
Two
Three
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There are repulsive forces between the reactants.
The concentration of HI decreases with time.
The concentration of the reactants is less than that of the product.
The reaction rate is decreasing with time.
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The physical state of the reactants.
The amount of the reactants.
The size of the container used.
The temperature at which the reaction is carried out.
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