Phosphoglucoisomerase interconverts glucose 6‑phosphate to, and from, glucose 1‑phosphate. glucose 6 - phosphate phosphoglucoisomerase ⇌ glucose 1 - phosphate glucose 6-phosphate⇌ 1-phosphate After mixing equal amounts of the two molecules, the solution achieved equilibrium at 25 ∘ C . 25 ∘C. The concentration at equilibrium of glucose 1‑phosphate is 0.01 M, 0.01 M, and the concentration at equilibrium of glucose 6‑phosphate is 0.19 M. 0.19 M. Calculate the equilibrium constant, K eq , Keq, and the standard free energy change, Δ G ∘ , ΔG∘, of the reaction mixture.

The equilibrium constant of the reaction is 0.0526 and standard Gibbs free energy of the reaction is -7.296 kJ/mol

Explanation:

For the given chemical equation:

The expression of for above equation follows:

We are given:

Putting values in above expression, we get:

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

where,

= Standard Gibbs free energy

R = Gas constant = 8.314 J/K mol

T = Temperature =

= Equilibrium constant of the reaction = 0.0526

Putting values in above equation, we get:

Hence, the equilibrium constant of the reaction is 0.0526 and standard Gibbs free energy of the reaction is -7.296 kJ/mol

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.