Acritical 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 the reaction atp(aq)+h2o(l)⟶adp(aq)+hpo2−4(aq) for which δ∘rxn=−30.5 kj/mol at 37.0 °c and ph 7.0. calculate the value of δ in a biological cell in which [atp]=5.0 mm, [adp]=0.70 mm, and [hpo2−4]=5.0 mm.

Answer : The value of is -49.2 kJ/mol

Explanation :

First we have to calculate the reaction quotient.

Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

The expression for reaction quotient will be :

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

Given:

= 5.0 mM

= 0.70 mM

= 5.0 mM

Now put all the given values in this expression, we get

Now we have to calculate the value of .

The formula used for is:

   ............(1)

where,

= Gibbs free energy for the reaction  = ?

=  standard Gibbs free energy  = -30.5 kJ/mol

R = gas constant =

T = temperature =

Q = reaction quotient =

Now put all the given values in the above formula 1, we get:

Therefore, the value of is -49.2 kJ/mol

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