SHOW ALL WORK PLEASE (15 points). The following are based on calculations for G,
ID: 586862 • Letter: S
Question
SHOW ALL WORK PLEASE
(15 points). The following are based on calculations for G, and G, at 370C·and pH 7.0 for hypothetical reactions. Fill in the table below using the value of R of 8.314 J/ mole K. Reaction AG, (J/mole K equilibrium ratio 1000/1 CD D-PE 3.35 Assume that reactions are at equilibrium, calculate G-when the following changes are made for the reactions and predict if there is an increase in product or reactan Reaction Increase in products or reactants Change made AG AB CD C-> D Add 100 A Remove 10 A Add 20 C Remove 5 CExplanation / Answer
For the given hypothetical reactions, the values of dGo and dG' would be as follows,
Reaction dGo (J/K.mol) equilibrium ratio
A --> B +10 49/51
B --> C -17803 1000/1
C --> D -3.35 100/1
D --> E +1786 1/2
dGo = -RTlnK
K = e^(-dGo/RT)
T = 37 oC + 273 = 310 K
when dGo = +10 J/K.mol
So, K = e^(-10/8.314 x 310) = 0.99611
equilibrium ratio (B/A) = 0.99611 x 100/1.99611 = 49.9%
when, equilibrium ratio = 1000/1
K = 1000
dGo = -8.314 x 310 ln(1000) = -17803 J/K.mol
Similarly others may be done
dG' and effect of reaction parameters
Reaction change mode dG' Increase in products or reactants
A ---> B Add 100 A -ve Increase in products
B ---> C Remove 10 A +ve Increase in reactants
C ---> D Add 20 C -ve Increase in reactants
C---> E Remove 5 C +ve Increase in reactants
The changes are according to the LeChatellier's principle, wherein when the state of equilibrium for a reaction is disturbed by adding or removing system parameter. The reaction will shift to that side so as to reduce the effect of that change and reestablish the state of equilibrium again.
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