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Wednesday, November 30

7:00 – 8:15

180 Bevier

AQ5 Bhagi

AQ6 Bhagi

AQ8 Bhagi

AQJ Blair

160 English

AQ2 Abadeer

AQ3 Abadeer

66 Library

AQ1 Abadeer

AQ4 Abadeer

AQB Barrick

101 Armory

AQ7 Barrick

AQ9 Barrick

AQA Barrick

Conflict Exam

5:30 – 6:45

161 Noyes Lab

K

at a given temperature, it is constant

K = [products]eqp

For solution chemistry

[reactants]eqr

K = Pproductsp

For gases

Preactantsr

or

Kc = [products]eqp

[reactants]eqr

K = Kc (RT)n

R = 0.08207

it changes until it = K

Q

is not constant

Q = [products]ip

For solution chemistry

[reactants]ir

Q = Pprod ip

For gases

Preact ir

if Q > K

reverse reaction

too much product initially

if Q < K

forward reaction

too much reactant initially

if Q = K

system at equilibrium

Write the expression for K for the reaction:

CaCO3 (s) CaO (s) + CO2 (g)

K = 0.0045

at 800oC

K

= PCO2

1 mol of CaCO3, 1 mol of CaO and 1 atm CO2

Q =

CaCO3

1

make more

- forward

CaO

b) reverse

1 mol of CaCO3 and 1 atm CO2

0

Q =

reaction table

ICE table

+ I2 (g)

2HI (g)

H2 (g)

Q = 02/(0.5)2

at 453oC,

calculate K

at equilibrium,

[H2] = 0.107 M

= 0.50

– x

x = 0.393

=

(0.786)2

=

54.3

= (2x)2

K =

[HI]2eq

[I2]eq

[H2]eq

(0.50–x)

(0.50–x)

(0.107)2

[I2] (M)

[HI] (M)

[H2] (M)

Initial

0.50

0.50

0.00

Change

- x

- x

+2x

2x

0.50 – x

0.50 – x

Equilibrium

K =

54.3

+ I2 (g)

2HI (g)

H2 (g)

K =

x = .782

54.3 =

(.224 + 2x)2

Q =

(.224)2

= .195

< K

x = .355

(.623 – x)

(.414 – x)

(.414)

(.623)

x =

-b ±

- 57.2x

50.3x2

+ 13.96

= 0

b2 – 4ac

2a

ax2

bx

c

[H2] (M)

[HI] (M)

[I2] (M)

Initial

.623

.414

.224

Change

- x

-x

+2x

Equilibrium

.623 - x

.414 - x

.224 + 2x

CH3OH (aq)

CH2O (aq) + H2 (aq)

K = 3.7 x 10-10 at 298 K

Starting with a 1.00 M solution of CH3OH,

what are the equilibrium concentrations ?

[CH2O] (M)

[H2] (M)

[CH3OH] (M)

0

Initial

1.00

0

-x

+x

+x

Change

Equilibrium

1.00 - x

x

x

CH3OH (aq)

CH2O (aq) + H2 (aq)

1.92 x 10-5

x 100 =

0.00182%

1.00

1.00 – 0.0000192

= 1.00

x = 1.92 x 10-5

K = 3.7 x 10-10

= x2

= x2

1.00

1.00 - x

1.00

very small

1.00 – x

[CH2O] (M)

[H2] (M)

[CH3OH] (M)

0

Initial

1.00

0

-x

+x

+x

Change

Equilibrium

1.00 - x

x

x

N2 O4 (g) 2 NO2 (g) Kc = 4.0 x 10-7

- If 0.1 mol of N2 O4 (g) is reacted in a 1.0 L , what
- is the equilibrium concentration of NO2 (g) ?
- 2.6 x 10-5M
- 1.2 x 10-2M
- 2.0 x 10-4M
- 4.0 x 10-7M
- 7.8 x 10-3M

FeSCN2+ (aq) Fe3+ (aq) + SCN- (aq)

K = 8.3 x 10-5

Calculate the equilibrium concentrations

when starting with 2.0 M FeSCN2+

8.3 x 10-5 = x2

x2

x = 0.0129

2.0 - x

2.0

0.0129

x 100% =

0.644%

2.0

5% approximation O.K.

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