Recitation Section 4 Answer KeyBiochemistry—Energy and GlycolysisWhy do we careThermodynamicsEnergy currencyGlycolysisRecitation Section 4 Answer Key February 22-23, 2006 Biochemistry—Energy and Glycolysis A. Why do we care In lecture we discussed the three properties of a living organism: metabolism, regulated growth, and replication. Today we will focus on metabolism and biosynthesis. 1. It was said in lecture that chemical reactions are the basis of life. Why do we say that? Being alive implies being able to change your state in response to a change in internal or environmental conditions. We discussed previously that any change in the observable characteristics of a cell begins as and is propagated by molecular interactions. Molecular interactions propagate the signal by changing the state of molecules, i.e. by reactions. 2. Why is metabolism required for life? A cell is subject to all laws of chemistry and physics, including the first and second law of thermodynamics. Changing the state of molecules dissipates energy along the way, so getting or making new energy is essential to life. The energy is then used for many purposes, including making the building blocks and precursors and then using them to build macromolecules that make up cells—biosynthesis. 3. Can an entity that performs no chemical reactions be considered “alive?” In general, no. But there are special cases of the cells that do not perform reactions right at the moment, but have the potential to perform reactions if they encounter particular conditions. Some examples of such cells are spores in nature or frozen permanents in laboratory. If they experience certain conditions, such as availability of food for spores, or defrosting and food source for frozen permanents, these cells will again perform metabolism. 4. Most reactions necessary for life are unfavorable, or do not proceed at an appreciable rate under physiological conditions. How do cells overcome this problem? Several mechanisms exist to allow necessary but unfavorable reactions to proceed or to speed up to levels required for cellular function. Below we explore the following mechanisms: -Enzymes, -concentration gradients, and -coupling unfavorable reactions with favorable ones, including -using the common energy currency, ATP. B. Thermodynamics 1. What is “free energy”? “Free energy” (defined by Gibbs, so we use the symbol G) is the total amount of energy in a system that can be used to do work. By definition, ∆G = “the total free energy of products” – “the total free energy of reactants”2. Where is this energy stored? The energy is stored in the bonds of the reactant and product molecules. We say that ∆G is a thermodynamic property, meaning that it is independent of the way that the conversion of reactants to products might proceed. 3. Based on how energy is stored in the molecules, explain why ∆G is independent of the path of the reaction. The energy is stored in the bonds. Regardless of how the reaction proceeds (all in one step, or in 10 steps, like glycolysis), the products will still look like the same exact molecules. Thus, the amount of energy stored in the bonds of the products will still be the same, and the difference in energy levels between reactants and products will still be the same. 4. If ∆G=0, the reaction is at equilibrium. What then is the meaning of the magnitude of ∆G? The magnitude of ∆G is the measure of the amount of work that can be done by a chemical reaction before it reaches equilibrium. 5. What is a favorable reaction? What would ∆G be for a thermodynamically favorable reaction? A favorable, or exergonic, reaction is one in which the energy state of reactants is higher than that of the products (∆G<0). 6. What is an unfavorable reaction? What would ∆G be for a thermodynamically unfavorable reaction? An unfavorable, or endergonic, reaction is the one in which the energy state of the products is higher than that of the reactants (∆G>0). 7. Not all thermodynamically favorable reactions proceed on their own. Why? Some reactions with negative ∆G still do not proceed at an appreciable rate. This is usually because some intermediate is in a significantly higher energy state than the reactants. The difference between the energy state of the reactants and such an intermediate is known as activation energy (Ea). 8. Catalysts overcome this problem. How do they do it? Catalysts (most often protein enzymes) lower the activation energy of the reaction, thus allowing the reaction to proceed. They sometimes accomplish this by physically positioning reactants in a way that brings parts of the molecules that will participate in the reaction in close contact.9. Is the equilibrium of the reaction affected by the action of a catalyst? Why or why not? The equilibrium of the reaction (relative concentrations of reactants and products) is not affected by the presence of the catalyst. This is because the equilibrium is determined by the amount of energy available to perform the work of converting reactants to products and vice versa. Since the energy is stored in the bonds, it is independent of the path the reaction takes, or the rate at which it occurs. 10. Is the rate of the reaction affected by the action of a catalyst? Why or why not? The rate of reaction is affected. Reactants reach the transition state due to random fluctuations in energy caused by molecular motion. If Ea is lowered, much less energy is required to reach it, so more molecules will be able to do so, and the rate of the reaction will increase. 11. Why can the direction in which a reaction proceeds be influenced by the relative concentration of reactants and products? If you have more molecules of a particular kind, it is more probable that some of them will reach the high energy state of the transition state. C. Energy currency Enzymes can not make thermodynamically unfavorable reactions proceed. But they do lower the activation energy of a reaction in both directions. 1. What strategy can a cell use to drive slightly thermodynamically unfavorable catalyzed reactions? How can this be achieved in a cell? As discussed above, skewing the concentrations in favor of reactants can drive such a reaction forward. This can be achieved by immediately siphoning off any newly formed products, thus maintaining the concentration gradient. Sometimes the reaction is just too
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