If for the C D reaction is +10 kJ/mol, show how you would calculate the ratio of D ΔG°’ ↔ to C at equilibrium. For the reaction E F, assume is 5 times as much F as E at equilibrium. How ↔ would you calculate for this reaction? What is the sign of for this reaction? ΔG°’ ΔG°’ What is the Keq for this reaction? If the for the reaction G H is +5 kJ/mol, in what direction will the reaction proceed ΔG°’ ↔ with the following starting concentrations? The starting concentration of G is 0.3 M and H is 0.3 M. The starting concentration of G is 0.3 M and H is 2.5 M.
If ΔG°’ for the C ↔ D reaction is +10 kJ/mol, show how you would calculate the ratio of D to C at equilibrium. For the reaction E ↔ F, assume is 5 times as much F as E at equilibrium. How would you calculate ΔG°’ for this reaction? What is the sign of ΔG°’ for this reaction? What is the Keq for this reaction? If the ΔG°’ for the reaction G ↔ H is +5 kJ/mol, in what direction will the reaction proceed with the following starting concentrations? The starting concentration of G is 0.3 M and H is 0.3 M. The starting concentration of G is 0.3 M and H is 2.5 M.
MetabolicControl11.06.16.docx