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UNCG KIN 292 - Types of Metabolic Reactions and Metabolic Reactions and Energy

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KIN 292 1st Edition Lecture 4 These are the notes from Professor Starnes’ lecture of Clinical Human Physiology. These come from the slideshows provided by the professor and include extra notes and explanations. Highlighted or bolded information are things that I believe to be information that is important to look over multiple times. The notes in red are my personal additions and quotes of Professor Starnes from the class lecture. Outline of Last Lecture I. Biomolecules:a. Molecules synthesized by living thingsb. Contain carbon, 4 unpaired electronsII. Four basic types:a. Carbohydratesb. Lipidsc. Amino acids and proteinsd. NucleotidesOutline of Current Lecture I. Types of Metabolic ReactionsII. Metabolic Reactions and EnergyCurrent LectureTypes of Metabolic Reactions- Metabolism- the sum of all chemical reactions occurring in a cell- Energy metabolism – main focus of Ch. 3o Reactions involved in energy storage and use. The basic principals chemical reactions apply to all machines, including the human bodyo Bioenergetics – the study of energy transfer in biological systems- Metabolism = chemical reactions in bodyo Anabolism Synthesis – energy must be put onto the reactionso Catabolism Breakdown – energy is given off when the reactions occur- Coupled Reactions – Some energy given off from catabolism is used for anabolic purposesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o Ex. A portion of the energy released during glucose oxidation (catabolism) can be used to synthesize ATPo Example of catabolic reactions providing energy to be used for anabolic reactionso Take in energy from outside (eating grass) materials breakdown and excreted as water, and nitrogenous waste.- Metabolism = chemical reactions in bodyo Many physiological systems are involved in making sure that metabolism can occur in an individual cell of a given organ.o Ex. When a decrease in ATP concentration is detected in cell, the cardiovascular system goes into action to increase the delivery of oxygen to that cello ATP levels have to remain constant under all conditionsCalorie and Joule are only units of measurement for energy o Energy expressed in calories (cal) or joules (J) 1 cal = 4.18 Jo Must have oxygen to go through the whole process, howmuch heat/energy is it producing/using?o 1 cal = energy required to raise 1 mL by 1°C. Heat is a formof energy that is released when substances are burned.Oxygen is required for thiso Calorimetry – the measurement of energy change is brieflydiscussed in Ch 21, page 606o Bomb calorimeter directly measures energy value of foodo There is a known value of water and volumeo Inside is a chamber that has oxygen and food that will be burned up. Shows how much energy is needed to kill caloriesWhat is Energy?- The Capacity to do Worko Work = Force x Distance (kg-m, foot-lb)o 1 kcal = 426.4 kg-m or 3087 ft-lb (100% efficient perfect machine where all energy is transferred directly to work – does not exist)- Power = F x D divided by Time (W/T) (watts)- Forms of Energy:o Kinetic energy Associated with motion Thermal, radiant, electromagnetic, electricalo Potential energy Stored energy Chemical, mechanical, nuclear, gravitationalLaws of Thermodynamics First Law of Thermodynamics:- Energy transfer- Energy cannot be created or destroyed, but is transformed from one form to another without being depleted.o Conservation of energy Illustrated as body transforms energy in food to heat, mechanical, and chemical energy- Heat will be given off Second Law of Thermodynamics:- Explains why energy is transferred- All of the energy of the Universe will inevitable be degraded to heat and the organization of matter will become totally randomized- Entropy (randomness) of a closed system will progressively increase and the amount of energy capable of performing work will diminish.- Nonrandom system (entropy low) contains energy by virtue of its orderliness - in becoming disordered (increase in entropy) work can be performed- The rhinoceros example from earlier is a closed system. It is taking from the environment.Second Law of Thermodynamics II: The transfer of energy in any spontaneous process always proceeds in a direction that decreases the capacity to do work.- Work may or may not have been accomplished during the decrease in capacity for work – it depends on whether the energy loss was connected to work – recall the mechanical box.- Some of the mechanical energy from balls moving to one side was transferred to electrical energy. The belt provided the coupling between the energy loss and energy gain. Without belt, only energy loss and none of it could be transferred.- The term free energy is used because this energy is available, or free, to do work. - As entropy increases, free energy decreasesEnergy Changes in Reactions- All reactions involve an exchange of energy- Molecules possess energy- Reactants possess more energy than productso reactants  products + energy- Change in energy of a reaction = Eo E = Ereactants – Eproducts- Putting previous 2 ΔE pictures togetherGoing from C to D can only occur if the reaction is coupled to A to B and ΔE1 is greater than ΔE2. 2nd Law thingC-D example: synthesis of ATPA-B example: a step (reaction) in the catabolism (breakdown) of glucose that yields ATP as a productActivation Energy - Transition stateo Reactant and product transformations are not sudden- Activation energy barrier- Energy of barrier = activation energy- Limits how fast a reaction goes- Level of required activation energy is reached then reaction will spontaneously occur to completion (2nd Law). Level of required activation energy not reached= no reaction happens- Bomb calorimeter. When temperature gets hot enough, activation energy barrier is overcome and all the substance burns to completionRole of Enzymes in Chemical Reactions- Enzymeso Proteins that are catalysts for reactions in biological systemso Catalysts increase the rates of chemical reactions- Enzymes function by decreasing the activation energy for a specific chemical reaction- Enzymes bind to a reactant (substrate). enzyme + substrate - ES - product +


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UNCG KIN 292 - Types of Metabolic Reactions and Metabolic Reactions and Energy

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