The standard free-energy change for this reaction in the direction written is 23.8 kJ/mol. The concentrationsof the three intermediates in the hepatocyte of a mammal are: fructose 1,6-bisphosphate,1.4X10-5 M; glyceraldehyde 3-phosphate, 3X10-6 M; and dihydroxyacetone phosphate, 1.6X10-5 M. At body temperature (37C), what is the actual free-energy change for the reaction

The actual free-energy change for the reaction  -8.64 kJ/mol.

Explanation:

The given reaction is as follows.

  Fructose 1,6-bisphosphate Glyceraldehyde 3-phosphate + DHAP

For the given reaction, is 23.8 kJ/mol.

As we know that,

Here,    R = 8.314 J/mol K,       T =

                                                    = (37 + 273) K

                                                    = 310.15 K

Fructose 1,6-bisphosphate = M

Glyceraldehyde 3-phosphate = M

DHAP = M

Expression for reaction quotient of this reaction is as follows.

    Reaction quotient =

        Q =

            =

Now, we will calculate the value of as follows.

                      =

                      = -8647.73 J/mol

                      = -8.64 kJ/mol

Thus, we can conclude that the actual free-energy change for the reaction  -8.64 kJ/mol.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

there are two significant figures.