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Today, 16:54

Consider the following metabolic reaction:Succinyl-CoA + Acetoacetate - --> Acetoacetyl-CoA + Succinate (delta) G = - 1.25 kJ/molThe (delta) G for the hydrolysis of Succinyl-CoA is - 33.9 kJ/mol. What is the (delta) G for the hydrolysis of Acetoacetyl-CoA: Acetoacetyl-CoA - --> Acetoacetate + CoAa. - 35.2 kJ/molb. - 32.7 kJ/molc. + 32.7 kJ/mold. none of the above

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  1. Today, 18:29
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    b. - 32.7 kJ/mol

    Explanation:

    For this metabolic reaction we have two coupled reactions taking place, which are:

    (1) Acetoacetyl-CoA - --> Acetoacetate + CoA

    (2) Succinyl-CoA + Acetoacetate - --> Acetoacetyl-CoA + Succinate

    So the overall variaton of free energy (ΔG°) for the metabolic reaction will be the sum of the individual free energy variations of each of the coupled reactions:

    ΔG°₁ + ΔG°₂ = ΔG°total.

    In this case, the ΔG°total is the result of the Succinul-CoA hydrolysis, which is - 33.9 kJ/mol. And we already have the variation of free energy for reaction (2), which is ΔG°₂ = - 1.25 kJ/mol. So with this we can obtain the value for ΔG°₁, which corresponds to the variation of free energy for the hydrolysis of Acetoacetyl-CoA.

    ΔG°₁ + (-1.25 kJ/mol) = ΔG°total.

    ΔG°₁ = ΔG°total - ΔG°₂

    ΔG°₁ = - 33.9 kJ/mol - (-1.25 kJ/mol)

    ΔG°₁ = - 33.9 kJ/mol - (-1.25 kJ/mol)

    ΔG°₁ = - 33.9 kJ/mol + 1.25 kJ/mol)

    ΔG°₁ = - 32.65 kJ/mol → rounding decimals → - 32.7 kJ/mol
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