Consider the fructose-1,6-bisphosphatase reaction. calculate the free energy change if the ratio of the concentrations of the products to the concentrations of the reactants is 21.3 and the temperature is 37.0 ° c ? δ g ° ' for the reaction is − 16.7 kj/mol .

The Gibbs free energy of the reaction is -8.82 kJ/mol

Explanation:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= standard Gibbs free energy = -16.7 kJ/mol = -16700 J/mol  (Conversion factor: 1kJ = 1000J)

R = Gas constant =

T = Temperature =

= Ratio of concentration of products and reactants = 21.3

Putting values in above equation, we get:

Hence, the Gibbs free energy of the reaction is -8.82 kJ/mol

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.