THERMOCHEMISTRY - Second and third laws: Entropy and Spontaneity
17 important questions on THERMOCHEMISTRY - Second and third laws: Entropy and Spontaneity
Is enthalpy alone a criterion of spontaneity?
T/F is entropy closely related to probability?
What is a microstate?
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Is Entropy a state of function?
Can entropy (S) be absolutely evaluated?
Is the entropy higher for larger or smaller atoms/molecules of the same type?
- It is larger
- because there is a lot more room to be random
T/F does compound of S increase with chemical complexity?
- True
- Because there are alot more atoms to rearrange
- molecules have more freedom to move
What is the change in entropy?
- ΔS = S(final) - S(initial)
- solid -> liquid (fusion)
- sans-serifliquid -> gas (evaporation)
- solid -> gas (sublimation)
If there is no phase change, what dictates the entropy?
- Temperature would dictate entropy
- When T increases = ΔS >0
- Kinetic energy Increase = more motion = more disorder
What is the second law of thermodynamics?
- In a spontaneous process, the entropy of the universe tends to increase
- ΔS(univ) = ΔS(sys)+ ΔS(sur) > 0
What is the third law of thermodynamics?
- The entropy of a pure perfect crystal is 0K is ZERO
- There is no disorder in a perfect system
What is the equation for the entropy of a reaction?
When you see a negative sign of ΔS is the given reaction always nonspontaneous?
- Examples in which this is not the case!
- liquid freezes below 0 (spontaneous)
- ΔS<0 liquid -> solid (reverse of fusion)
How to determine the ΔS(surr)?
- The sign depends on the direction of the heat flow!
- ENDOTHERMIC : ΔH(sys) >0
- heat from surroundings declines
- entropy of surroundings decline
- EXOTHERMIC : ΔH(sys) < 0
- heat in surroundings increases
- entropy of surroundings increases
When finding the magnitude of ΔS(sur), what formula do we use?
What is free energy?
What is the equation for when ΔS(univ) is spontaneous?
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