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Kinesiology 2230A/B Lecture Notes - Lecture 1: Flavin Adenine Dinucleotide, Creatine Kinase, Exergonic Reaction

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31 Oct 2017

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Western University

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Kinesiology 2230A/B

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Document Summary

Nutritional sources: fat and carbohydrate are all made of c, h, and o, protein is adding n on top. 3: coa acetyl coenzyme a acetyl group carrier, fad flavin adenine dinucleotide hydrogen transfer, active the enzyme (cid:449)ithout it the e(cid:374)zy(cid:373)e (cid:449)o(cid:374)"t (cid:449)ork. Exercising: when creatine kinase is present, pcr gets brakes down to creatine and pi and releases energy, the energy is used to bond pi with adp to form atp, and atp provides energy by breaking down pi. Recovery: at rest, aerobic metabolism regenerate atp, then the atp here is used to provide energy to bind creatine and pi with presence of creatine kinase (reversible) to replenish pcr. Adp accumulation is slower than pcr depletion: adp + adp atp + amp myokinase. 7: whe(cid:374) pyru(cid:448)ate does(cid:374)"t gets produ(cid:272)ed too fast fro(cid:373) la(cid:272)tate, Depends on the intensity of exercising: if moderate exercising, the path goes relatively slow so pyruvate can get into mitochondria to metabolic aerobically.

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Related Questions

At constant pressure, the combustion of 10.0 g of C2Hg(g) releases 518 kJ of heat. What is AH for the reaction given below? 2 C2H6(g) +- 7 O2(g) rightarrow 4 CO2(g) + 6 H2O(l). -779 kJ -1560 kJ -86.1 kJ -3120 kJ Use the information provided to determine Delta H degree r times n for the following reaction: CH4(g) + 3 Cl2(g) rightarrow CHCI3(I) + 3 HCI(g) Delta H degree r times n = ? -217 kJ -335 kJ +662 kJ +117 kJ -151 kJ Choose the reaction that illustrates Delta H degree f for NaHCO3. Na(s) + 2 H(g) + C(s) + 3 O(g) rightarrow NaHCO3 (s) Na(s) + H2(g) + C(s) + O2(g) rightarrow NaHCO3 (s) Na+(aq) + H2O (I) + CO2 (g) rightarrow NaHCO3 (s) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) rightarrow NaHCO3 (s) Na+(aq) + HCO3 -1 (aq) rightarrow NaHCO3 (s) Use the standard reaction enthalpies given below to determine Delta H degree r times n for the following reaction: 4 SO3(g) rightarrow 4 S(s) + 6 O2(g) Delta H degree r times n = ? Given: SO2(g) rightarrow S(s) + O2(g) Delta H degree r times m = +296.8 kJ 2 SO2(g) + O2(g) rightarow 2 SO3(g) Delta H degree r times n = -197.8 kJ -494.6 kJ -791.4 kJ 1583 kJ -293.0 kJ -692.4 kJ Which of the following statements is TRUE? State functions do not depend on the path taken to arrive at a particular state. Energy is neither created nor destroyed, excluding nuclear reactions. Delta Hr times r can be determined using constant pressure calorimetry. Delta H r times n can be determined using constant volume calorimetry. All of the above are true. How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) rightarrow Al2O3(s) + 2 Fe(s) Delta H degree r times n = 852 kJ 01.51 times 103 kJ 241 kJ 0482 kJ 4.20 x 103 kJ 753 kJ Given w = 0, an endothermic reaction has the following. - Delta H and + Delta E Delta H and -Delta E - Delta H and -Delta E + Delta H and +Delta E Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? 10.0 g ethanol, Celharol = 2.42 J/g degree C 10.0 g Ag, CAg = 0.235 J/g degree C 10.0 g Au, CAu = 0.128 J/g degree C 10.0 g Fe, CFe = 0.449 J/g degree C 10.0 g H2O, CHO = 4.18J/g degree C Which of the following processes is endothermic? a hot cup of coffee (system) cools on a countertop the vaporization of rubbing alcohol the chemical reaction in a "hot pack" often used to treat sore muscles the freezing of water the combustion of propane

Show transcribed image text At constant pressure, the combustion of 10.0 g of C2Hg(g) releases 518 kJ of heat. What is AH for the reaction given below? 2 C2H6(g) +- 7 O2(g) rightarrow 4 CO2(g) + 6 H2O(l). -779 kJ -1560 kJ -86.1 kJ -3120 kJ Use the information provided to determine Delta H degree r times n for the following reaction: CH4(g) + 3 Cl2(g) rightarrow CHCI3(I) + 3 HCI(g) Delta H degree r times n = ? -217 kJ -335 kJ +662 kJ +117 kJ -151 kJ Choose the reaction that illustrates Delta H degree f for NaHCO3. Na(s) + 2 H(g) + C(s) + 3 O(g) rightarrow NaHCO3 (s) Na(s) + H2(g) + C(s) + O2(g) rightarrow NaHCO3 (s) Na+(aq) + H2O (I) + CO2 (g) rightarrow NaHCO3 (s) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) rightarrow NaHCO3 (s) Na+(aq) + HCO3 -1 (aq) rightarrow NaHCO3 (s) Use the standard reaction enthalpies given below to determine Delta H degree r times n for the following reaction: 4 SO3(g) rightarrow 4 S(s) + 6 O2(g) Delta H degree r times n = ? Given: SO2(g) rightarrow S(s) + O2(g) Delta H degree r times m = +296.8 kJ 2 SO2(g) + O2(g) rightarow 2 SO3(g) Delta H degree r times n = -197.8 kJ -494.6 kJ -791.4 kJ 1583 kJ -293.0 kJ -692.4 kJ Which of the following statements is TRUE? State functions do not depend on the path taken to arrive at a particular state. Energy is neither created nor destroyed, excluding nuclear reactions. Delta Hr times r can be determined using constant pressure calorimetry. Delta H r times n can be determined using constant volume calorimetry. All of the above are true. How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) rightarrow Al2O3(s) + 2 Fe(s) Delta H degree r times n = 852 kJ 01.51 times 103 kJ 241 kJ 0482 kJ 4.20 x 103 kJ 753 kJ Given w = 0, an endothermic reaction has the following. - Delta H and + Delta E Delta H and -Delta E - Delta H and -Delta E + Delta H and +Delta E Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? 10.0 g ethanol, Celharol = 2.42 J/g degree C 10.0 g Ag, CAg = 0.235 J/g degree C 10.0 g Au, CAu = 0.128 J/g degree C 10.0 g Fe, CFe = 0.449 J/g degree C 10.0 g H2O, CHO = 4.18J/g degree C Which of the following processes is endothermic? a hot cup of coffee (system) cools on a countertop the vaporization of rubbing alcohol the chemical reaction in a "hot pack" often used to treat sore muscles the freezing of water the combustion of propane