<p>Does hydrolysis and condensation both require an initial input of energy?</p>
<p>Do all chemical reactions require an initial input of energy to get started?</p>
<p>Is this initial input of energy in the form of free energy? Is heat free energy?</p>
<p>It would be appreciated if anyone can answer these questions for me.</p>
<p>Well yes to first and second question. There is something called the activation energy which is the minimum energy required for a reaction to occur.
For hydrolysis it is a non-spontaneous process so it takes more energy to make the reaction actually happen. Same as for condensation although ‘spontaneous’ is different under different temperatures and pressure situations.
are you talking about Gibb’s Free Energy? You can only define Gibb’s Free Energy as deltaG=deltaH-T*deltaS So I don’t get your question.</p>
<p>I guess my real question would be “what is activation energy?” Is it free energy? I am studying biology and in my book it says reactants absorb free energy to initiate. So what is this free energy? Can it be any form of energy like heat?</p>
<p>Or is heat not free energy? If so, why can reactants absorb heat to initiate reactions?</p>
<p>I don’t know what you mean by ‘free energy’. Type the part that mentions about it in your book. As for activiation energy it is simply the minimum amount of energy needed to start a particular reaction. For spontaneous reactions under STP it is low while for reactions like the electrolysis of water it is high.</p>
<p>“free energy” or, more accurately, “Gibbs free energy” is the amount of energy available in a system capable of doing work. It can be in the form of heat, and most of the reactions initiated in chemistry classes involves adding heat to the reactants. Enzymes lower the amount of activation energy required, but all reactions require activation energy.</p>
<p>Thanks for clearing things up.</p>
<p>To answer your other question, heat is only a component of free energy.<br>
In the formula G = H - ST, heat energy would be represented by H (enthalpy, or the total potential energy of a system). The other factor in calculating Gibbs Free Energy is S (entropy, or the basis of the second law of Thermodynamics).</p>
<p>Gibb’s free energy has nothing to do with exergonic/endergonic (exothermic/endotheric) reactions, which I believe is the core of your questions. Instead it determines the probability that a chemical reaction will occur spontaneously at any given temperature and pressure.</p>
<p>Your question about hydrolysis/condensation leads me to ask you if you are studying energy coupling?</p>
<p>Yeah, my textbook mentions energy coupling. When energy made through catabolic pathways are used to fuel energy consuming anabolic pathways right? Also, it is how free energy released from exergonic reactions is used to power endergonic reactions.</p>
<p>rite… i haven’t seen any chemistry stuff since 9th grade. boy am i gonna not enjoy that class… :(</p>