A reaction has a ΔG of 5.6 kcal/mol. Circle the correct answer and state why each incorrect answer is true. The reaction could be coupled to a power endergonic reaction with a ΔG of +8.8 kcal/mol. The reaction is nonspontaneous and endergonic. 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. During a laboratory experiment, you discover that an enzyme-catalyzed reaction has a ΔG of kcal/mol. If you double the amount of enzyme in the reaction, what will be the ΔG for the reaction? Briefly explain your choice below. A-40 kcal/mol 20 kcal/mol.
Added by Salvador H.
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6 kcal/mol. This means that the reaction is nonspontaneous and endergonic, as it requires an input of energy to proceed. Now, let's consider the statement: "The reaction could be coupled to power an endergonic reaction with ΔG of +8.8 kcal/mol." This statement is Show more…
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