Calculation of δg′° from an equilibrium constant calculate the standard free-energy change for each of the following metabolically important enzyme-catalyzed reactions, using the equilibrium constants given for the reactions at 25 °c and ph 7.0. ( a ) glutamate + oxaloacetate aspartate aminotranferase ⇌ aspartate + α -ketoglutarate k ′ eq = 6.8 ( b ) dihydroxyacetone phosphate triose phosphate isomerase ⇌ glyceraldehyde 3 -phosphate k ′ eq = 0.0475 ( c ) fructose 6 -phosphate + atp phosphofructokinase ⇌ fructose 1 , 6 -bisphosphate + adp k ′ eq = 254

Answer :

(a) The value of for the reaction is -4.7 kJ/mol

(b) The value of for the reaction is 7.55 kJ/mol

(c) The value of for the reaction is -13.7 kJ/mol

Explanation :

The relation between the equilibrium constant and standard Gibbs free energy is:

where,

= standard Gibbs free energy

R = gas constant = 8.314 J/K.mol

T = temperature =

 = equilibrium constant

Now we have to calculate the value of for the following reactions.

(a)    

Thus, the value of for the reaction is -4.7 kJ/mol

(b)    

Thus, the value of for the reaction is 7.55 kJ/mol

(c)    

Thus, the value of for the reaction is -13.7 kJ/mol

hurricanes form when warm, moist air from the ocean surface quickly rises into the atmosphere and forms storm clouds and rain. when the clouds are formed, heat is released which warms the cool air in the upper regions of the atmosphere so that the cycle can continue. which two phases of the water cycle are repeated in this process?

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