4. A reaction has a ?G of -5.6 kcal/mol. Which of the following would most likely be true? ? The reaction could be coupled to power an endergonic reaction with a ?G of +8.8 kcal/mol. ? The reaction is nonspontaneous. ? To take place, the reaction would need to couple to ATP hydrolysis. ? The reaction would result in products with a greater free-energy content than in the initial reactants. ? The reaction would proceed by itself but might be very slow.
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6 kcallmol). This means that the reaction is spontaneous and will release energy. Show more…
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Which of the following reactions could be coupled to an endergonic reaction with $\Delta G=+3.56 \mathrm{kJ} / \mathrm{mol}$ ? (a) $\mathrm{A} \rightarrow \mathrm{B}, \Delta G=+6.08 \mathrm{k} / \mathrm{mol}$ (b) $C \rightarrow D, \Delta G=+3.56 \mathrm{kJ} / \mathrm{mol}$ (c) $E \rightarrow F, \Delta G=0 \mathrm{k} / \mathrm{mol}$ (d) $G \rightarrow H, \Delta G=-1.22 \mathrm{kJ} / \mathrm{mol}$ (e) $1 \rightarrow 1, \Delta G=-5.91 \mathrm{kJ} / \mathrm{mol}$
Choose a suitable reaction from the answer choices that could be coupled to the reaction given here: A + B <-> C + D (Delta G = -8.7 kcal/mole) A + F <-> G + H (Delta G = +10.2 kcal/mole) E + F <-> G + H (Delta G = -5.4 kcal/mole) C + F <-> G + H (Delta G = +8.3 kcal/mole) B + F <-> G + H (Delta G = -5.4 kcal/mole) C + F <-> G + H (Delta G = +9.7 kcal/mole)
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