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***Please note, this is ONE question with multiple parts to it. This is NOT 4 different...

***Please note, this is ONE question with multiple parts to it. This is NOT 4 different questions.*** If something is unclear, please be specific in the feedback what exactly that needs to be clarified instead of writing "Need more subject knowledge".

Consider the following biological oxidation reduction reaction: NADH (aq)+H+(aq)→NAD+(aq)+H2(g) Using the chemical convention for the standard state concentration [H+]o the standard Gibbs energy of reaction is: ΔrGo=-21.8 kJ/mol.

Part A. Calculate the standard Gibbs energy change for the chemical reaction ΔrGo' i.e. assuming the biochemical convention for [H+]o. Give you answer in units of J/mol.

ΔrGo' i=???

Part B. Aessume the reaction has the following conditions: [NADH]=1.5*10-2M, [H+]=3.00x10-5M, [NAD+]=4.6x10-3M, and PH2=0.010bars. Calculate ΔrG for for this reaction using these conditions and the chemical convention. Give you answer in Joules per mole.

ΔrG=???

Part C.Calculate ΔrG for for this reaction using the conditions given in part C and the biochemical convention. Give you answer in Joules per mole.

ΔrG=???

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