2. The standard Gibbs formation energy of ions
Saturated
Solution of B
CB,S
Diluted
Solution of B
CB=1.0 mol.L-1
Stable simple
substances
Pure
Compounds B

3. About biochemical standard state and the thermodynamic equilibrium constant
CΘ(H+)=[H+]=10-7mol.dm-3
A+B ↔ C+ xH+
No effect on

5. 6.6 Effect of environmental conditions on the chemical reaction equilibrium
(1) Temperature
G-H equation
The van’t Hoff equation

6. Le Chatelier’s principle
Endothermic: increasing temperature favours the products
Exothermic: increasing temperature favours the reactants
Le Chatelier’s principle
A system at equilibrium, when subjected to a disturbance,
responds in a way to minimise the effects of the disturbance.

7. a plot of - ln K against 1/T has a slope of ΔrHm/R.
Integration equation:
a plot of - ln K against 1/T has a slope of ΔrHm/R.

8. Approximate Calculation about Equilibrium at different temperature
Tr=298K
Approximation

9. Increasing temperature
benefit the reaction
Decreasing temperature benefit the reaction
Turning temperature

10. (2)Pressure Only related to temperature
Only related to temperature, too

11. Le chatelier principle
KP , KC not related to P
B, the gaseous substance
P↑, Kx↑, move to right
Kx related to P:
Le chatelier principle

12. (3) Effect of inert gases on chemical equilibrium
Gases do not take part in the reaction, such as N2
( )T,V no change/ ( )T,P similar to p decreasing =0
No effect on Kn ↑ ↑
Equilibrium move to right

13. 6.6 Contemporary chemical equilibrium
The product of the previous reaction is the reactant of the latter reaction
At equi. state

14. =0 (1),(2)
1-x x x x
X=0.039

15. Biochemical reactions

16. G+Pi↔G6P+H2O 11.6 0.5 ATP+H2O↔ADP+Pi -32.5 -30.9 298K
ΔG0/KJ.mol-1
ΔH0/KJ.mol-1
G+Pi↔G6P+H2O
ATP+H2O↔ADP+Pi
G+ATP↔G6P+ADP
Kc=4630
Kc= K

17. Coupling reactions METABOLIC CYCLES

18. The overall reaction Glucose+2Pi+2ADP↔2Lactate+2ATP+2H2O
ΔG0=-124.4kJ.mol-1
Glucose(s)+6O2↔6CO2(g)+6H2O(l)
ΔG0= kJ.mol-1
ΔH0= kJ.mol-1

19. Direct synthesis of ATP
In 1961, Peter Mitchell proposed that the synthesis of ATP occurred due to a coupling of the chemical reaction with a proton gradient across the membrane
He received a Nobel Prize for his work

20. Mechanisms of direct synthesis of ATP
ATP+H2O↔ADP+Pi kJ.mol-1
ADP+Pi ↔ ATP+H2O
nH+(out)↔nH+(in)
n=3
A pH differential of one unit gives a free energy change of kJ.mol-1
Membrane potential -100mV

21. Homework
Y: P ; P139 42, 43
Discussion how the temperature, pressure affect the Haber reaction equilibrium, give out the approach increasing the yields of NH3.
N2+3H2↔2NH3
The Haber process,
also called the Haber–Bosch process
Haber
Bosch