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Questions and Answers
What is the consequence of the second law of thermodynamics in a closed system?
What is the consequence of the second law of thermodynamics in a closed system?
- Entropy decreases over time
- Entropy increases over time (correct)
- Entropy remains unchanged
- Entropy remains constant over time
What is the condition for a reaction to be spontaneous at all temperatures?
What is the condition for a reaction to be spontaneous at all temperatures?
- ∆H must be zero and ∆S must be zero
- ∆H must be positive and ∆S must be negative
- ∆H must be negative and ∆S must be positive (correct)
- ∆H must be positive and ∆S must be positive
Which of the following is a violation of the second law of thermodynamics?
Which of the following is a violation of the second law of thermodynamics?
- Ice formation at a constant temperature and pressure
- Heat flowing from a cold object to a hot object
- A room spontaneously organizing itself into a perfectly clean state (correct)
- Rusting of iron
What is the relationship between the spontaneity of a process and the value of ∆G?
What is the relationship between the spontaneity of a process and the value of ∆G?
What is the significance of ∆G = 0 in a reaction process?
What is the significance of ∆G = 0 in a reaction process?
What is the unit of Gibbs free energy?
What is the unit of Gibbs free energy?
Which of the following factors does not affect the spontaneity of a reaction according to Gibbs free energy?
Which of the following factors does not affect the spontaneity of a reaction according to Gibbs free energy?
What is the scenario in which entropy remains unchanged?
What is the scenario in which entropy remains unchanged?
What is the equation that correctly represents the relationship between Gibbs free energy, enthalpy, and entropy?
What is the equation that correctly represents the relationship between Gibbs free energy, enthalpy, and entropy?
What is the significance of a negative ∆G value?
What is the significance of a negative ∆G value?
What is the relationship between the equilibrium constant (K) and the spontaneity of a process?
What is the relationship between the equilibrium constant (K) and the spontaneity of a process?
What is the effect of an endothermic process on the enthalpy change (∆H)?
What is the effect of an endothermic process on the enthalpy change (∆H)?
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Study Notes
Second Law of Thermodynamics
- States that entropy of the universe increases in spontaneous processes and remains unchanged in equilibrium processes
- Entropy represents disorder or randomness in a system
- In energy transfer or transformation, some energy becomes lost as heat
- Heat always flows from a hot object to a cold object
- Irreversibility of natural processes is a principle of increasing entropy
Entropy
- Measure of disorder or randomness in a system
- Increases over time in a closed system
Predicting Spontaneity
- Gibbs free energy (∆G) is used to predict spontaneity of a process
- ∆G < 0 indicates a spontaneous process at constant temperature and pressure
- ∆G = 0 indicates equilibrium
- K > 1 indicates a spontaneous process
Types of Processes
- Rusting of iron is a spontaneous process
- Melting of ice cubes at -50°C and 1 atm is non-spontaneous
- Arranging books on a shelf by height does not show increasing entropy
- Endothermic process absorbs heat from the surroundings
- Ice formation is an example of a non-spontaneous process
Gibbs Free Energy
- ∆G = ∆H – T∆S is the equation correctly representing the relationship between Gibbs free energy, enthalpy, and entropy
- ∆G is typically measured in Joules (J)
- Negative ∆G indicates a spontaneous reaction
- Factors affecting spontaneity of a reaction: temperature (T), enthalpy change (∆H), and entropy change (∆S)
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