Question

Consider the malate dehydrogenase reaction from the citric acid cycle. Given the listed concentrations, calculate the free energy change for this reaction at energy change for this reaction at 37.0 ∘ C (310 K). Δ G ∘ ′ for the reaction is + 29.7 kJ/mol . Assume that the reaction occurs at pH 7.

Consider the malate dehydrogenase reaction from the citric acid cycle. Given the listed concentrations, calculate the free energy change for this reaction at energy change for this reaction at 37.0°C (310 K). AG' for the reaction is +29.7 kJ/mol. Assume that the reaction occurs at pH 7. malate] = 1.19 mm oxaloacetate) = 0.230 mM (NAD) = 260 mM (NADH) = 1.0 x 10mM AG: kJ-mol

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Answer 1

24 UU OY 25 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 359-006 WEEK 52 10.00 11.00 12.00 1.00 2.00 TUESDAY. DECEMBER solution 9.00 We know that Chemical reaction for conversion Malate + NA NADT & oxaloacetate + NADH and the expression of keq for above equation is given by - keq = [Oxalo acetatě 3 x [NADHT - [ Malate] x [NAD + ] According to the Question [ Malate ] = 1.19 mm [ oxaloa cetate J = 0.230 mm I NAD+] = 260 MM [NADH) = 10 x 102 mm From Equation A 3.00 4.00 5.00 6.00 7.00 Keg = 0.230 x 100 1.19 x 260 23 309.4 = Cleanliness is happiness. 0.0743

JANUARY 2019 M T W T F S S M T W T F S S 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 360-005 WEEK 52 26 WEDNESDAY. DECEMBER we know the Relation between Gibbs free 9.00 Energy and Equilibrium constant area 10.00 AG = AGO + RT In keg - 11.00 where AGO = 29.7 KJ /mol = 29700 J/mol & Girent 1200 R = Gas Constant (8.314 J/kmol) 1.00 T = temperature = 37°c or 30k 20 and we have Keq = 0.0743 300 on suostituting above values in Equation B 400 we get 5.00 LG = 29700 + (8.314 X 310 x ln 0.0743) ___y = २०२५ 7/M/ - 23.024 kJ/mol Hence Gibbs free Energy = 23.024 kJ/mol 6.00