The final reaction of glycolysis catalyzes hydrolysis of a phosphate from phosphoenolpyruvate, yielding pyruvate. This is an exergonic reaction with a ΔG of -61.9 kJ/mol. This reaction is coupled to the synthesis of ATP from ADP and phosphate. The ΔG of hydrolysis of ATP to ADP and Pi is -30.5 kJ/mol. What is the ΔG for the coupled reaction? Based on these calculations, define reaction coupling. Why is this reaction irreversible?
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9 kJ/mol - ΔG for the hydrolysis of ATP to ADP and Pi: -30.5 kJ/mol ** Show more…
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The ΔG°' for phosphoenolpyruvate hydrolysis is -61.9 kJ/mol, while the ΔG°' for ATP hydrolysis is -30.5 kJ/mol. What is the overall ΔG°' when ATP synthesis (the reverse reaction of ATP hydrolysis) is coupled with phosphoenolpyruvate hydrolysis? 0.0 kJ/mol +31.4 kJ/mol -31.4 kJ/mol +92.4 kJ/mol -92.4 kJ/mol
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In the metabolism of glucose, the first step is the conversion of glucose to glucose 6 -phosphate: glucose $+\mathrm{H}_{3} \mathrm{PO}_{4} \longrightarrow$ glucose 6 -phosphate $+\mathrm{H}_{2} \mathrm{O}$ $\Delta G^{\circ}=13.4 \mathrm{kJ} / \mathrm{mol}$ Because $\Delta G^{\circ}$ is positive, this reaction does not favor the formation of products. Show how this reaction can be made to proceed by coupling it with the hydrolysis of ATP. Write an equation for the coupled reaction and estimate the equilibrium constant for the coupled process.
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