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Transcript of Unless otherwise stated, all images in this file have been reproduced from: Blackman, Bottle,...
Unless otherwise stated, all images in this file have been reproduced from:
Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 2007 (John Wiley)
ISBN: 9 78047081 0866
Slide 2/21
e CHEM1002 [Part 2]
A/Prof Adam Bridgeman (Series 1)Dr Feike Dijkstra (Series 2)
Weeks 8 – 13
Office Hours: Monday 2-3, Friday 1-2Room: 543ae-mail: [email protected]: [email protected]
Slide 3/12
e
Lecture 6:• Physical States and Phase Changes• Blackman Section 7.3
Entropy
Lecture 7:• Entropy• Blackman Section 8.4
Lecture 8:• Crystal Structures• Blackman Chapter 7, Section 7.4 (pages 259-265)
Slide 4/12
e
H2O(s) H2O(l) DH = +6.02 kJ mol-1
• The temperature of the surroundings is also important!
Spontaneous Reactions?
• In which direction is this reaction spontaneous?
At -10 °C: liquid solid
At 10 °C: solid liquid
(exothermic)
(endothermic)
Slide 5/12
e
Twarm Twarm
Thermal Equilibration
Thot Tcold
• Clearly, energy (heat) will move from the hotter body to the cooler body. Overall energy is constant.
ENTROPY may be thought of as this tendency for energy to spread out as far as possible.
The appropriate definition of thechange in entropy (S) is:
Derivation of this equation in CHEM2402
?
Δ = qST
Slide 6/12
e Energy Spreading Out…
Energy can be spread out in two main ways:• the molecules and their energy can be spread out further, or• the energy can be spread across more molecules
Slide 7/12
e
NO
NO2
N2O4
Entropy and Molecular Complexity
• Entropy increases as molecule grows more complex.
animations
Slide 8/12
e Amount of Entropy (S)• In many cases, the relative entropy of two different
systems can be understood intuitively.
S(gas) >> S(solid)
S(solid+liquid) < S(solution)
S(gas+liquid) > S(solution)
S(3 mol) > S(2 mol)
S(C2H6) > S (CH4)
Energy spreads further in gas
Energy localised in solid
Energy spreads further in gas
Entropy amount of substance
More bonds to spread energy around
Slide 9/12
x Which Has Higher Entropy?
• Which has the higher entropy in each of the following pairs?
(a) 1 mol of SO2(g) or
(b) 1 mol of CO2(s) or 1 mol of CO2(g)
(c) 3 mol of O2 or 2 mol of O3(g)
(d) 1 mol of KBr(s) or 1 mol of KBr(aq)
(e) Seawater in midwinter (2 0C) or in midsummer (23 0C)
more atoms
gas > solid
more molecules
solution > solid
higher T
1 mol of SO3(g)
Slide 10/12
e
DfusS
Entropy: Qualitative
• More disordered = higher S• For given substance: • Same substance:
meltingpoint
T
Ent
ropy
(S)
boilingpoint
Solid
Liquid
Gas
DvapS
(increasing vibrations)
(increasing translations)
(increasing speeds)
Sliquid > SsolidSgas > > higher T → higher S
Slide 11/12
x Practice Examples1.When one mole of ice melts to liquid at 0 °C,
A. The entropy of the system decreases.B. The entropy of the system remains the same.C. The entropy of the system increases.D. The order of the system increases. E. None of the above
2. The entropy of a chemical system will usually increase whenA. A molecule is broken down into two or more smaller
fragments.B. A reaction occurs that results in an increase in the moles
of gas.C. A solid changes to a liquid.D. A liquid changes into a gas.E. All of the above
Slide 12/12
e Summary: Entropy,Learning Outcomes - you should now be able to:
• Complete the worksheet• Explain what entropy is to a non-science friend• Predict whether entropy will increase or
decrease in a chemical or physical process• Apply the entropy concept qualitatively to
explain direction of phase change
Next lecture:
• Crystal structures