BIOCHEMISTRY
ENZYMES AND METABOLISM
|
Question
[CLICK ON ANY CHOICE TO KNOW THE RIGHT ANSWER]
|
|
|
The reaction will release more energy than was needed to form the reaction.
|
|
|
Energy from the reaction can be used to do work.
|
|
|
Energy is absorbed by the reaction which then can be used to power other reactions.
|
|
|
Energy is absorbed within the reaction and distributed unevenly throughout the molecule.
|
Detailed explanation-1: -A negative ∆G means that the reactants, or initial state, have more free energy than the products, or final state. Exergonic reactions are also called spontaneous reactions, because they can occur without the addition of energy.
Detailed explanation-2: -Because DG is a measure of how favorable a reaction is, it also relates to the equilibrium constant. A reaction with a negative DG, is very favorable, so it has a large K. A reaction with a positive DG is not favorable, so it has a small K. A reaction with DG = 0 is at equilibrium.
Detailed explanation-3: -However, whether the entropy of the system increases or decreases during a reaction, Delta G of the exothermic reactions is negative.
Detailed explanation-4: -A chemical reaction with a positive ∆G means that the products of the reaction have a higher free energy than the reactants (see the right panel of Figure 2). These chemical reactions are called endergonic reactions, and they are NOT spontaneous.