The standard free-energy change of the reactionphosphoenolpyruvate ADP-pyruvate + ATPis ΔG =-7.50 kcal. If the reaction is initiated with 6.0 millimole/L of ADP, 6.0 millimole/L ofphosphoenolpyruvate, 6.0 millimole/L of ATP, and 0.0 millimole/L of pyruvate, what will thefinal concentrations be?

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Asked Apr 22, 2019
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The standard free-energy change of the reaction
phosphoenolpyruvate ADP-
pyruvate + ATP
is ΔG =-7.50 kcal. If the reaction is initiated with 6.0 millimole/L of ADP, 6.0 millimole/L of
phosphoenolpyruvate, 6.0 millimole/L of ATP, and 0.0 millimole/L of pyruvate, what will the
final concentrations be?
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The standard free-energy change of the reaction phosphoenolpyruvate ADP- pyruvate + ATP is ΔG =-7.50 kcal. If the reaction is initiated with 6.0 millimole/L of ADP, 6.0 millimole/L of phosphoenolpyruvate, 6.0 millimole/L of ATP, and 0.0 millimole/L of pyruvate, what will the final concentrations be?

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Expert Answer

Step 1

From the given value of change in Gibbs free energy of the process, the equilibrium constant can be calculated as:

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Step 2

The value of R = 2 cal/Kmol

Since, the value of Gibbs free energy is standard, thus temperature = T = 25 0C = (25+273 ) K = 298 K

Thus, the equilibrium constant of the process can be calculated using equation (1):

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Step 3

The ICE table for the given react...

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