Short answer responses please! 6. Explain in quantitative terms the circumstance

Question

Short answer responses please! 6. Explain in quantitative terms the circumstances under which the following reaction can proceed. Citrate ?isocitrate 10°=+13.3 kJ/mol 7. In glycolysis, the enzyme pyruvate kinase catalyzes this reaction: Phosphoenolpyruvate + ADP Epyruvate + ATP Given the information below, show how you would calculate the equilibrium constant for this reaction. (R 8.315 J/mol K; T-298 K) Reaction 1) ATP ADP+P Reaction 2) phosphoenolpyruvate lpyruvate+P G-30.5 kJ/mol 10° =-61,9 kJ/mol 8. Explain what is meant by the statement: "Standard free-energy changes are additive Give an example of the usefulness of this additive property in understanding how cells carry out thermodynamically unfavorable chemical reactions. 9. GivenG for each of the following reactions, 1. ATP BADP+P 2. glucose 6-phosphate Wglucose + P 30.5 kJ/mol 13.8 kJ/mol show how you would calculate the standard free-energy change (LG") for the reaction: 3. ATP+ glucose Hglucose 6-phosphate + ADP 10. Why is the actual free energy b) of hydrolysis of ATP in the cell different from the standard free energy y 11. What is an oxidation? What is a reduction? Can an oxidation occur without a simultaneous reduction? Why or why not?

Explanation / Answer

Sinc eyou have posted multiple long answer questions, I am going to answer first two. I hope it helps. Thanks

1. A reaction for which delta G'° is positive, can proceed under conditions in which delta G is negative. From the relationship
?G = ?G'° + RT ln [product]
[reactant]
It is clear that if the concentration of product is kept very low, the logarithmic term becomes negative and delta G can then have a negative value.

2. The reaction is the sum of reaction 2 and the reverse of reaction 1.

Therefore,

?G'° = -31.4 kJ/mol.

?G'° = -RT ln Keq' ln Keq'

-?G'°/RT= 31.4 kJ/mol / [(8.315 J/mol·K)(298 K)] ln Keq'

= 12.672 K' = 3.19 x 105

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