A critical reaction in the production of energy to do work or drive chemical rea

Question

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems Is the hydrolysis of adenosine triphosphate. ATP. to adenosine diphosphate. ADP, as described by ATP[aq] + H_20(l) rightarrow ADP(aq?) + HPO^2-_4 (aq) for vwhich DeltaG*_nm - - 30.5 Kj/mol at 37.0 Degree C and pH 7.0 Calculate the value of Delta G_nnm in a biologcal cell in which [ATP] = 5.0 mM, [ADP] = 0.60 mM, and [HP0_4^2-| = 50 mM kJ/mol Is the hydrolysis of ATP spontaneous under these conditions?

Explanation / Answer

delG= Chage in Gibbs energy= delG0+ RTlnQ

where Q= [ADP] [HPO4-2]/ [ATP]= 0.6*5/5= 0.6 mM=6*10-4M

lnQ= ln(6*10-4)=-7,42

R= 8.314 Jmol T= 37+273.15=310.15K

delG= 30.5*1000+8.314*.310.1515*(-7.42)=11370.54J/mol=11..37 Kj/mol

since delG is +ve, the reaction is spontaneous in the reverse reaction.It is not spontaneous

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