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. a) calculate the equilibrium constant k at t=298k using the chemical convention for the standard state concentration [h+]o. b) calculate the equilibrium constant k' at t=298k using the biochemical convention for the standard state concentration [h+]o.
c) calculate the standard gibbs energy change for the chemical reaction deltargo' i. e. assuming the biochemical convention for [h+]o. give you answer in units of j/mol. d) assume the reaction has the following conditions: [nadh]=1.5*10-2m, [h+]=3.00x10-5m, [nad+]=4.6x10-3m, and ph2=0.010bars. e) calculate deltarg for for this reaction using these conditions and the chemical convention. give you answer in joules per mole. f) calculate deltarg for for this reaction using the conditions given in part e and the biochemical convention. give you answer in joules per mole.