Question

3. Let’s now consider a slightly different reaction, a reaction in solution:

Glucose (aq)--->Fructose (aq)

a). Give the expression of the equilibrium constant K in terms of the concentration of glucose and fructose in the solution. What kind of reference states do you assume for the two solutes here?

b). If someone determined that this conversion has ∆rG0=+1.7kJmol-1 in aqueous solution. If you start off with a solution of 0.1M of pure glucose in the solution, what would be final concentration of glucose and fructose respectively assuming the two can interconvert and reach equilibrium.

d) In reality, do you think glucose will be converted to fructose in water? What prevents the conversion? You may look up google to learn more about structural difference between glucose and fructose.

4.Consider the reaction CO(g) + H2O (g) <---> CO2(g) + H2(g) , K = 0.0611 at 2000K. A reaction mixture initially contains CO(g) partial pressure of 1344torr and H2O partial pressure 1760torr and 2000K. Calculate the equilibrium partial pressures of each of the products after the reaction reaches equilibrium (you may use “simplifying approximations” in solving the equation).

Answer 1

a) K= [Concentraion of Fructose/[Concentraion of Glucose]

b)c) Since the gibbs free energy is positive this reaction is not feasible. In real life catalyst such as lithium or certain enzymes are used to catalyze this reaction.