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# Lab Manual & Schedule Tutorial Formula sheet - PowerPoint PPT Presentation

Lab Manual & Schedule Tutorial Formula sheet Many Different Exchange Opportunities available for Windsor Students. There will be an Student Exchange Information Fair on Thursday, January 10 from 11am to 2pm in the CAW Student Centre.

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• Lab Manual & Schedule

• Tutorial

• Formula sheet

• Many Different Exchange Opportunities available for Windsor Students. There will be an Student Exchange Information Fair on Thursday, January 10 from 11am to 2pm in the CAW Student Centre

### Chapter 7: Chemical EquilibriumChapter 9 in the 7th edition

1. Extent of reaction (ξ):

The amount of reactants being converted to products. Its unit is mole.

Consider: A ↔ B

Assume an infinitesimal amount dξ of A turns into B,

dnA = -dξ

On the other hand, dnB = dξ

• Why do we need a new quantity?

consider a generic reaction: 2A ↔ 3B

• In a very general way, the extent of reaction is calculated

as dξ = dnA/vA (where vA is the stoichiometric number of the reactant A, which is negative for the reactant!!)

Example 1: N2(g) + 3H2(g) ↔ 2NH3(g)

when the extent of reaction changes from ξ = 0 to ξ = 1.0 mole, what are the changes of each reagent?

Solution: identify vj:

v(N2) = -1; v(H2) = -3; v(NH3) = 2.

since dξ = 1.0 mole,

dn(N2) = -1x1.0 mole = -1.0 mole,

dn(H2) = -3x1.0 mole = -3.0 moles,

dn(NH3) = 2x1.0 mole = 2.0 moles,

Example 2: CH4(g) + Cl2(g) ↔ CHCl3(l) + HCl(g), in which the amount of reactant Cl2(g) decreases by 2 moles. What is the extent of the reaction?

Solution:

the slope of the Gibbs energy plotted against the extent of reaction:

ΔrG =

here Δr signifies a derivative

• A reaction for which ΔrG < 0 is called exergonic.

• A reaction for which ΔrG > 0 is called endergonic.

• ΔrG < 0, the forward reaction is spontaneous.

• ΔrG > 0, the reverse reaction is spontaneous.

• ΔrG = 0, the reaction is at equilibrium!!!

• Consider the reaction A ↔ B

initial amount nA0 nB0

final amount nAf nBf

Ginitial = uBnB0 + uAnA0

Gfinal = uBnBf + uAnAf

ΔG = Gfinal - Ginitial = (uBnBf + uAnAf ) – (uBnB0 + uAnA0 )

= uB(nBf- nB0) + uA (nAf - nA0) = uBΔξ + uA(-Δξ)

= (uB - uA )Δξ

ΔrG = = uB - uA

When uA > uB, the reaction A → B is spontaneous.

When uB > uA, the reverse reaction (B → A) is spontaneous.

When uB = uA, the reaction is spontaneous in neither direction (equilibrium condition).

7.2 The description of equilibrium Gibbs energy

1. Perfect gas equilibrium:

A(g)↔ B(g)

ΔrG = uB – uA

• At equilibrium, Gibbs energyΔrG = 0, therefore

Note: The difference in standard molar Gibbs energies of the products and reactants is equal to the difference in their standard Gibbs energies of formation, thus,

ΔrGθ = ΔfGθ(B) - ΔfGθ(A)

Equilibrium for a general reaction Gibbs energy

Example: 2A + B ↔ C + 3D

• The reaction Gibbs energy, ΔrG, is defined in the same way as discussed earlier:

where the reaction quotient, Q, has the form:

Q = activities of products/activities of reactants

in a compact expression Q = Π αjνj

vj are the corresponding stoichiometric numbers; positive for products and negative for reactants.

vA = -2; vB = -1; vC = 1; vD = 3

• Justification of the equation Gibbs energy

dG = ∑ujdnj

Assuming that the extent of reaction equals dξ,

one gets dnj = vjdξ

then dG = ∑ujdnj

= ∑ujvjdξ

(dG/dξ) = ∑ujvj ΔrG = ∑ujvj

because uj = ujθ + RTln(aj)

ΔrG = ∑{vj(ujθ + RTln(aj))}

= ∑(vjujθ) + ∑vj(RTln(aj))

= ΔrGθ + RT ∑ln(aj)vj

= ΔrGθ + RT ln (∏(aj)vj) = ΔrGθ + RT ln (Q)

• Again, we use Gibbs energyK to denote the reaction quotient at the equilibrium point,

K = Qequilibrium = (∏ajvj)equilibrium

K is called thermodynamic equilibrium constant. Note that until now K is expressed in terms of activities)

Example: calculate the quotient for the reaction: A + 2B ↔ 3C + 4D

Solution: first, identify the stoichiometric number of each reactant:

vA = -1, vB = -2, vC = 3, and vD = 4.

At the equilibrium condition:

Examples of calculating equilibrium constants Gibbs energy

• Consider a hypothetical equilibrium reaction

A(g) + B(g) ↔ C(g) + D(g)

While all gases may be considered ideal. The following data are available for this reaction:

Compound μθ(kJ mol-1)

A(g) -55.00

B(g) -44.00

C(g) -54.00

D(g) -47.00

Calculate the value of the equilibrium constant Kp for the reaction at 298.15K.

Solution:

Example 2: Using the data provided in the data section, calculate the standard Gibbs energy and the equilibrium constant at 25oC for the following reaction

CH4(g) + Cl2(g) ↔ CHCl3(g) + HCl(g)

Solution: (chalkboard)

ΔfGθ(CHCl3, g) = -73.66 kJ mol-1

ΔfGθ(HCl, g) = - 95.30 kJ mol-1

ΔfGθ(CH4, g) = - 50.72 kJ mol-1