[webassignbuddy]

5. The equilibrium constant of a reaction is 3.91e+02 at 466 K and 7.82e+03 at 556 K. Determine the following for this reaction:

a) ΔHº = 71.7 kJ/mol
b) ΔSº = 203.6

c) What is the value of the equilibrium constant at 511 K?

R ln K = [ΔSº - ΔHº](1/T)
(8.314) ln K = [203.6 J - 71,700 J](1/511 K)
(8.314) ln K = (-71496.4 J)(1/511 K)
(8.314) ln K = -139.914 J/K
ln K = -139.914/8.314
ln K = -16.828
K = e^(-16.828)
K = 1/e^(16.828)
K = 4.9 x 10^-8 at 511 K

^ Is that right? And what about the one below

6. Consider the reaction

TiO2(s) 2C(graphite) 2Cl2(g) TiCl4(g) 2CO(g)

Determine the following at 298 K:

a) ΔHº = -39.54 kJ/mol (CORRECT)
b) ΔSº = 241.34 J/mol-K (CORRECT)
c) ΔGº = -111.6 kJ/mol (CORRECT)
d) What is log K at 298K (log K = ln K/2.3026)?

How do I figure out part d?

[sjb]

5. The equilibrium constant of a reaction is 3.91e+02 at 466 K and 7.82e+03 at 556 K. Determine the following for this reaction:

a) ΔHº = 71.7 kJ/mol
b) ΔSº = 203.6

c) What is the value of the equilibrium constant at 511 K?

R ln K = [ΔSº - ΔHº](1/T)
(8.314) ln K = [203.6 J - 71,700 J](1/511 K)
(8.314) ln K = (-71496.4 J)(1/511 K)
(8.314) ln K = -139.914 J/K
ln K = -139.914/8.314
ln K = -16.828
K = e^(-16.828)
K = 1/e^(16.828)
K = 4.9 x 10^-8 at 511 K

^ Is that right? And what about the one below

Check your units in the first step of part c. Does it make sense that the rate constant is significantly different to that at the other temps?

6. Consider the reaction

TiO₂(s) 2C(graphite) 2Cl₂(g)  TiCl₄(g) 2CO(g)

Determine the following at 298 K:

a) ΔHº = -39.54 kJ/mol (CORRECT)
b) ΔSº = 241.34 J/mol-K (CORRECT)
c) ΔGº = -111.6 kJ/mol (CORRECT)
d) What is log K at 298K (log K = ln K/2.3026)?

How do I figure out part d?

Do you know any relationships between K and ΔG°?

[webassignbuddy]

5. The equilibrium constant of a reaction is 3.91e+02 at 466 K and 7.82e+03 at 556 K. Determine the following for this reaction:

a) ΔHº = 71.7 kJ/mol
b) ΔSº = 203.6

c) What is the value of the equilibrium constant at 511 K?

R ln K = [ΔSº - ΔHº](1/T)
(8.314) ln K = [203.6 J - 71,700 J](1/511 K)
(8.314) ln K = (-71496.4 J)(1/511 K)
(8.314) ln K = -139.914 J/K
ln K = -139.914/8.314
ln K = -16.828
K = e^(-16.828)
K = 1/e^(16.828)
K = 4.9 x 10^-8 at 511 K

^ Is that right? And what about the one below

Check your units in the first step of part c. Does it make sense that the rate constant is significantly different to that at the other temps?

6. Consider the reaction

TiO₂(s) 2C(graphite) 2Cl₂(g)  TiCl₄(g) 2CO(g)

Determine the following at 298 K:

a) ΔHº = -39.54 kJ/mol (CORRECT)
b) ΔSº = 241.34 J/mol-K (CORRECT)
c) ΔGº = -111.6 kJ/mol (CORRECT)
d) What is log K at 298K (log K = ln K/2.3026)?

How do I figure out part d?

Do you know any relationships between K and ΔG°?

For part c of #5, the units are supposed to be in Joules, no?
Are yous saying that my answer to part c is wrong?

this is due in 2 hours
I'm too young to be stressing out like this

[webassignbuddy]

Oh wait!!
For 5c, the equation I should be using is:

R ln K = ΔSº - ΔHº(1/T)
ln K = [ΔSº - ΔHº/T]/R
ln K = [203.6 - 71700/511]/8.314
ln K = [203.6 - 140.313112]/8.314
ln K = 63.286888/8.314
ln K = 7.61208660091
K = e^(7.61208660091)
K = 2022.49383538
K = 2.022 x 10³

That's the answer for part c!

[webassignbuddy]

Part d would be...

1. ΔGº = -RT ln K
-111.6 kJ = -(0.008314)(298) ln K
-111.6 kJ = (-2.477572) ln K
-111.6 kJ/-2.477572 = ln K
45.0440996266 = ln K

2. log K = ln K/2.3026
log K = 45.0440996266/2.3026
log K = 19.56