chemistry 102(01) spring 2014

17-1CHEM 102, Fall 2014 LA TECH

Instructor: Dr. Upali Siriwardane

e-mail: upali@latech.edu

Office: CTH 311

Phone 257-4941

Office Hours: M,W 8:00-9:30 & 11:00-12:30 am;

Tu,Th,F 8:00 - 10:00 am. or by appointment.

Test Dates: 10:00-11:15 am., CTH 328

Chemistry 102(02) Fall 2014

September 23, 2014 (Test 1): Chapter 13

October 16, 2014 (Test 2): Chapter 14 &15

November 11, 2014 (Test 3) Chapter 16 &17

November 13, 2014 (Make-up test) comprehensive:

Chapters 13-17

Chapter 6. Thermochemistry

6.1 Chemical Hand Warmers 2316.2 The Nature of Energy: Key Definitions 2326.3 The First Law of Thermodynamics: There Is No Free Lunch 2346.4 Quantifying Heat and Work 2406.5 Measuring for Chemical Reactions: Constant-Volume Calorimetry2466.6 Enthalpy: The Heat Evolved in a Chemical Reaction at Constant

Pressure 249

6.7 Constant-Pressure Calorimetry: Measuring 2536.8 Relationships Involving

2556.9 Determining Enthalpies of Reaction from Standard Enthalpies of Formation

2576.1 0 Energy Use and the Environment 263

Chapter 17. Free Energy and Thermodynamics17.1 Nature’s Heat Tax: You Can’t Win and You Can’t Break Even 769

17.2 Spontaneous and Nonspontaneous Processes 771

17.3 Entropy and the Second Law of Thermodynamics 773

17.4 Heat Transfer and Changes in the Entropy of the Surroundings 780

17.5 Gibbs Free Energy 784

17.6 Entropy Changes in Chemical Reactions: Calculating 788

17.7 Free Energy Changes in Chemical Reactions: Calculating 792

17.8 Free Energy Changes for Nonstandard States: The Relationship

between and 798

17.9 Free Energy and Equilibrium: Relating to the Equilibrium Constant

What forms of energy are found in the Universe?mechanical thermalelectrical Lightnuclearmass: E = mc2

others yet to discover

What is 1st Law of Thermodynamics

Eenergy is conserved in the Universe

All forms of energy are inter-convertible and conserved

Energy is neither created nor destroyed.

What exactly is DH?Heat measured at constant pressure qp Chemical reactions exposed to atmosphere

and are held at a constant pressure. Volume of materials or gases produced can

change.

What is the internal energy change (DU) of a system? DU is part of energy associated with changes in atoms, molecules and subatomic particles

Etotal = Eke + E pe + DU DU = heat (q) + w (work) DU = q + w DU = q -P DV; w =- P DV

Heat measured at constant volume qv

Chemical reactions take place inside a closed chamber like a bomb

calorimeter.

Volume of materials or gases produced can not change. ie: work = -PDV=

DU = qv + w

qv = DU + o; w = 0

DU = qv = DU(internal energy )

How is Internal Energy, DU measured?

EnthalpyHeat changes at constant pressure

during chemical reactionsThermochemical equation. eg.

H2 (g) + O2 (g) ---> 2H2O(l) DH =- 256 kJ; DH is called the enthalpy of reaction.if DH is + reaction is called endothermicif DH is - reaction is called exothermic

The thermodynamic property related to randomness is ENTROPY, S.

Product-favored processes: final state is more DISORDERED or RANDOM than the original.

Spontaneity is related to an increase in randomness.

Reaction of K with water

Entropy, S

Physical Process” S[H2O(l)] > S[H2O(s)] at 0° C.

DGo = DHo - T DSo

1. If DH is negative it helps product to be favored2. If DS is positive it helps product to be favored 3. If DG is negative reaction is product favored Gibbs free energy change = difference between the enthalpy of a system and the product of its absolute temperature and entropypredictor of spontaneity Total energy change of the system -

energy lost in disordering the system

Gibbs Free Energy, G

Thermodynamics Standard States The thermodynamic standard state of a substance is

its most stable pure form under standard pressure (1 atm) and at some specific

temperature (25 ºC or 298 K)

superscript circle is used to denote a thermodynamic quantity that is under standard state conditions:

ΔH = ΔH°ΔS = ΔS°ΔG = ΔG°

Hydrogen ΔHof

(kJ/mol)ΔGo

f (kJ/mol) So (J/mol K)

H2 (g) 0 0 130.7H (g) 218.0 203.2 114.7

H2O (l) -285.8 -237.1 69.9H2O (g) -241.8 -228.6 188.8H2O2 (l) -187.8 -120.4 109.6

Standard Thermodynamic Data

f - Standard Enthalpy of Formation

f - Standard Free Energy of Formation

- Standard Free Energy of Formation

Standard Molar Entropy Values

Chemical Thermodynamicsspontaneous reaction – reaction which

proceed without external assistance once started

chemical thermodynamics helps predict which reactions are spontaneous

Will the rearrangement of a system decrease its energy?

If yes, system is favored to react — a product-favored system.

Most product-favored reactions are exothermic.Often referred to as spontaneous reactions.“Spontaneous” does not imply anything about time for

reaction to occur. Kinetic factors are more important for certain reactions.

Thermodynamics

1) Give the definitions of the following:a) Enthalpy (H):

b) Enthalpy change of a thermo-chemical reaction (DH):

c) Entropy of a substance (S): d) Entropy change of a chemical reaction(DS): e) Thermodynamic Standard State(0):

Laws of Thermodynamics

Zeroth: Thermal equilibrium and temperature

First : The total energy of the universe is constant

Second : The total entropy (S) of the universe is always increasing

Third : The entropy(S) of a pure, perfectly formed crystalline substance at absolute

zero is zero

2) Give the definitions of the following:

a) Zeroth Law of thermodynamics:

b) First Law of thermodynamics:

c) Second Law of thermodynamics:

d) Third Law of thermodynamics:

Why is it necessary to divide Universe into System and SurroundingUniverse = System + Surrounding

system surroundings

universe

Boundary?

Types of Systems

Isolated system

no mass or energy exchange

Closed system

only energy exchange

Open system

both mass and energy exchange

Universe = System + Surrounding

Why is it necessary to divide Universe into System and Surrounding

3) Why we need to divide universe into surroundings and system for thermodynamic calculations?

Give the signs of the DH (heat) and DS (disorder) and DG ( free energy) when system lose or gain them.

DH (heat)

DS (disorder)

DG ( free energy)

Second Law of ThermodynamicsIn the universe the ENTROPY cannot decrease for

any spontaneous processThe entropy of the universe strives for a

maximumin any spontaneous process, the entropy of the

universe increasesfor product-favored processDSuniv = DSsys + DSsurr

DSuniverse = ( Ssys + Ssurr) > 0 DSuniv = entropy of the UniverseDSsys = entropy of the SystemDSsurr = entropy of the Surrounding

universe

system surroundings

Entropy of the UniverseVarious ways Dsuniv could become +

DSuniv = DSsys + DSsurr

Dsuniv DSsys DSsurr

+ + ++ +(DSsys>DSsurr) - + + (DSsurr>DSsys)

4) Explain the ways that DS of the universe, DSuniv could be +.

DSuniv = DSsys + DSsurr

Entropy and Dissolving

5) Assign a sign to the entropy change for the following systems.

a) mixing aqueous solutions of NaCl and KNO3 together:

b) spreading grass seed on a lawn: c) raking and bagging leaves in the fall: d) shuffling a deck of cards:

e) raking and burning leaves in the fall:

Expansion of a GasThe positional

probability is higher when particles are dispersed over a larger volume

Matter tends to expand unless it is restricted

Gas Expansion and Probability

Entropies of Solid, Liquidand Gas Phases

S (gases) > S (liquids) > S (solids)

6) Taking following examples explain how disorder is related to a measuring positional probability) or dispersion among the allowed energy states?

a) Expansion of gases: Two gas molecules trapped in two vessels with a tube with a stop cock.

6) Taking following examples explain how disorder is related to a measuring positional probability) or dispersion among the allowed energy states.

b) Distribution of Kinetic energy at 0, 25 and 100°C for O2

Entropy and Molecular Structure

Entropy, S

Entropies of ionic solids depend on coulombic attractions.

(J/K•mol)

MgO 26.9

NaF 51.5

Qualitative Guidelines for Entropy Changes

Entropies of gases higher than liquids higher than solids

Entropies are higher for more complex structures than simpler structures

Entropies of ionic solids are inversely related to the strength of ionic forces

Entropy increases when making solutions of pure solids or pure liquids in a liquid solvent

Entropy decrease when making solutions of gases in a liquid

Entropy of a Solution of a Gas

7) Arrange following in the order of increasing entropy?• a) C(s) (diamond)

• b) C(s) (graphite)

• c) O2(g)

• d) CO2(g)

• e) CO(g)

• f) Hg(l)

Entropy Change

Entropy (DS) normally increase (+) for the following

changes:i) Solid ---> liquid (melting) +ii) Liquid ---> gas +iii) Solid ----> gas most +iv) Increase in temperature +v) Increasing in pressure(constant volume, and

temperature) +vi) Increase in volume +

Qualitative prediction of DS of Chemical Reactions Look for (l) or (s) --> (g) If all are gases: calculate DnDn = Sn (gaseous prod.) - S n(gaseous react.)N2 (g) + 3 H2 (g) --------> 2 NH3 (g) Dn = 2 - 4 = -2If Dn is - DS is negative (decrease in S)If Dn is + DS is positive (increase in S)

Predict DS!

2 C2H6(g) + 7 O2(g)--> 4 CO2(g) + 6H2O(g)

2 CO(g) + O2(g)-->2 CO2(g)

HCl(g) + NH3(g)-->NH4Cl(s)

H2(g) + Br2(l) --> 2 HBr(g)

8) Taking following physical and chemical changes qualitatively predict the sign of DS.

a) 2H2O (g) ------> 2 H2O (l) b) 2H2O (g) ------> 2 H2 (g) + O2 (g) c) N2 (g) + 3 H2 (g) ------> 2 NH3 (g)

Entropy Changes for Phase Changes

For a phase change, DSSYS = qSYS/T

(q = heat transferred)Boiling Water

H2O (liq) H2O(g)DH = q = +40,700 J/mol

mol•J/K 109+ = K 373.15

J/mol 40,700 = Tq = SD

9) How is entropy related to the heat and temperature?

Phase TransitionsHeat of Fusionenergy associated with phase transition solid-to-

liquid or liquid-to-solidDGfusion = 0 = DHfusion - T DSfusion

0 = DHfusion - T DSfusion

DHfusion = T DSfusion

Heat of Vaporizationenergy associated with phase transition gas-to-

liquid or liquid-to-gasDHvaporization = T DSvaporization

10) The normal boiling point of benzene is 80.1°C and heat of evaporation (∆H°vap)is 30.7 kJ/mol. Calculate the ∆Ssurr (in J/K mol) for the evaporation of benzene.

Can calc. that DHo

rxn = DHosystem = -571.7 kJ

2 H2(g) + O2(g) 2 H2O(liq)DSo

sys = -326.9 J/KEntropy Changes in the Surroundings

q = systemsurrgssurroundin

K 298.15J/kJ) kJ)(1000 (-571.7 - = gssurroundin

= +1917 J/K

2nd Law of Thermodynamics

2 H2(g) + O2(g) 2 H2O(liq)DSo

sys = -326.9 J/KDSo

surr = +1917 J/KDSo

uni = +1590. J/KThe entropy of the universe is increasing, so

the reaction is product-favored.

2nd Law of Thermodynamics

Gibbs Free Energy, GDSuniv = DSsurr + DSsys

Multiply through by (-T)-TDSuniv = DHsys - TDSsys

-TDSuniv = DGsystem

Under standard conditions —

DGo = DHo - TDSo

D S univ = -D H sys

T + D S sys

Gibbs Free Energy, G DGo = DHo - T DSo

Gibbs free energy change = difference between the enthalpy of a system and

the product of its absolute temperature and entropy

predictor of spontaneity Total energy change for system -

energy lost in disordering the system

11) Define the following:a) Gibbs Free Energy (G): b) Gibbs Free Energy change for a reaction (DG):

c) How is DGsys is related to DSuni and temperature?

The sign of DG indicates whether a reaction will occur spontaneously.

+ Not spontaneous

0 At equilibrium

- Spontaneous

The fact that the effect of DS will vary as a function of temperature is important.

This can result in changing the sign of DG.

Free energy, DG

The sign of DG indicates whether a reaction will occur spontaneously.

Therefore Ecell value have to be + (positive) for spontaneous redox reaction

DG = -nFEcell

n = number of electrons transferred

F = Faraday constant ((96500 C/mol)

Ecell = E½(cathode)- E½(anode)

DG and Ecell

How do you calculate DG at different T and PDG = DGo + RT ln Q Q = reaction quotientat equilibrium DG = 00 = DGo + RT ln K DGo = - RT ln KIf you know DGo you could calculate K or

vice versa.

Nerst Equation, since DG = -nFEcell

11) Define the following: d) How you decided from the sign of DG whether and

chemical reaction is? i) Spontaneous ii) Never take place iii) Equilibrium e) How is Gibbs Free Energy change (DG°) related to Ecell:

f) How is non standard (DG) related to (DG°) and Q (reaction quotient)

11) Define the following:g) How is standard (DG°) related to Keq (equilibrium constant)?

Gibbs Free Energy, G

DGo = DHo - TDSo

DHo DSo DGo Reactionexo(-) increase(+) - Prod-favoredendo(+) decrease(-) + React-

favoredexo(-) decrease(-) ? T dependentendo(+) increase(+) ? T

dependent

12) Predict the DGsys changes for different signs of DHsys and DSsys at low/high temperatures for the equation:

DGsys = DHsys - TDSsys

DGsys DHsys - DTDSsys

chemistry 102(01) spring 2014

la tech

free energy changes

forms of energy

conserved energy

nature of energy

energy use

duinternal energy

gibbs free energy

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