ANATOMY AND PHYSIOLOGY: AN INTEGRATIVE A
4th Edition
ISBN: 9781265949440
Author: McKinley
Publisher: MCG
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Textbook Question
Chapter 3.1, Problem 1WDYL
Both the movement of Na+ down its concentration gradient and the movement of an electron from a higher energy to a lower energy state are examples of (a) potential energy or (b) kinetic energy?
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The distribution of Na* ions across a typical biological membrane is 10 mmol/dm3
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The stated difference in concentration MUST be maintained by coupling to
reactions that have at least your calculated difference of Gibbs energy.
Ans: 6.8 kJ/mol
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Chapter 3 Solutions
ANATOMY AND PHYSIOLOGY: AN INTEGRATIVE A
Ch. 3.1 - Both the movement of Na+ down its concentration...Ch. 3.1 - Muscle contraction is an example of what form of...Ch. 3.1 - Prob. 3WDYLCh. 3.2 - Prob. 4WDYLCh. 3.2 - For a biochemical reaction that involves simple...Ch. 3.2 - What molecule is formed from exergonic reactions...Ch. 3.2 - Explain what occurs when the equilibrium is...Ch. 3.2 - Explain the effect a fever would have on chemical...Ch. 3.3 - What is the relationship of enzymes and activation...Ch. 3.3 - What is the active site of an enzyme and how does...
Ch. 3.3 - What is the mechanism of enzyme action, including...Ch. 3.3 - Explain how enzymes are generally named.Ch. 3.3 - How do changes in substrate concentration,...Ch. 3.3 - How are enzymes regulated through competitive and...Ch. 3.3 - Prob. 15WDYLCh. 3.3 - Prob. 16WDYLCh. 3.4 - Prob. 17WDYLCh. 3.4 - Prob. 18WDYLCh. 3.4 - Prob. 19WDYLCh. 3.4 - Prob. 20WDYLCh. 3.4 - Prob. 21WDYLCh. 3.4 - Prob. 22WDYLCh. 3.4 - Prob. 23WDYLCh. 3.4 - Prob. 24WDYLCh. 3.4 - Prob. 25WDYLCh. 3.4 - Prob. 26WDYLCh. 3.4 - Prob. 27WDYLCh. 3.4 - Prob. 28WDYLCh. 3 - Energy in ATP is used to power skeletal muscle...Ch. 3 - Prob. 2DYKBCh. 3 - Prob. 3DYKBCh. 3 - ATP inhibits phosphofructokinase by binding to an...Ch. 3 - All of the following are accurate about enzymes...Ch. 3 - Prob. 6DYKBCh. 3 - Prob. 7DYKBCh. 3 - All stages of cellular respiration are decreased...Ch. 3 - Prob. 9DYKBCh. 3 - Prob. 10DYKBCh. 3 - Prob. 11DYKBCh. 3 - Describe the different ways of classifying...Ch. 3 - Prob. 13DYKBCh. 3 - Describe the structure and mechanism of enzymes.Ch. 3 - Prob. 15DYKBCh. 3 - Prob. 16DYKBCh. 3 - In general terms, explain the fate of pyruvate if...Ch. 3 - Describe how oxygen becomes part of water during...Ch. 3 - Identify the source of carbon in carbon dioxide.Ch. 3 - Prob. 20DYKBCh. 3 - Prob. 1CALCh. 3 - Prob. 2CALCh. 3 - Another challenge to a patient with impaired...Ch. 3 - Prob. 4CALCh. 3 - Prob. 5CALCh. 3 - Prob. 1CSLCh. 3 - Prob. 2CSLCh. 3 - What occurs to the amount of product formed in a...
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- A certain reaction with an activation energy of 195 kJ/mol was run at 555 K and again at 575 K . What is the ratio of f at the higher temperature to f at the lower temperature.arrow_forwardThe formation of maltose, a disaccharide, from two glucose molecules, is not energetically favorable. However, if this reaction is coupled with the hydrolysis of ATP, the reaction occurs more favorably. Maltose + H2O = 2 Glucose , ΔG'o = -15.5 KJ/mol or -3.7 kcal/mol a. Determine if the coupled reaction will occur spontaneously at standard state through calculating the Gibbs Free Energy of Reaction. b. Calculate the equilibrium constant for each individual reaction, and for the coupled reaction (using free energy of reaction). Show that the equilibrium constant for the coupled reaction equals the equilibrium constants for the individual reactions multiplied together. c. If the reaction medium contains the following chemical species at their given concentrations (298 K and 1.0 atm, pH = 7.0), will the reaction proceed in the forward or the reverse direction? [Maltose] = [Glucose] = 10.0 mM; [ATP] = 5.0 mM; [ADP] = [Pi] = 20 mMarrow_forwardOf the three thermodynamic quantities, enthalpy, free energy, and entropy, which provides the most useful indicator of spontaneity in a reaction? Explain.arrow_forward
- For this reaction: 6CO2 + 6H2O → C6H12O6 + 6O2, the products have 2760 kJ/mole more free energy than the reactants. So, which of the following statements best describes the reaction? a The reaction is endergonic because it converts molecules with less free energy to those with more free energy. b The reaction is exergonic because it converts molecules with less free energy to those with more free energy. c The reaction is exergonic because it converts molecules with more free energy to those with less free energy d The reaction is endergonic because it converts molecules with more free energy to those with less free energy.arrow_forwardGastric juice (pH 1.5) is produced by pumping HCl from blood plasma (pH 7.4) into the stomach. Calculate the amount of free energy required to concentrate the H+ in 1 L of gastric juice at 37 °C. Under cellular conditions,how many moles of ATP must be hydrolyzed to provide this amount of free energy? The free-energy change for ATP hydrolysis under cellular conditions is about −58 kJ/mol . Ignore the effects of the transmembrane electrical potential.arrow_forwardConsider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneousarrow_forward
- What do the following indicators tell you about whether a reaction can proceed as written? (a) The standard free-energy change is positive. (b) The free-energy change is positive. (c) The reaction is exergonicarrow_forwardDespite the thermal stability of covalent bonds in physiological systems, some of these bonds are sensitive to energy input from external sources. The molecule can absorb heat from the environment without changing its chemical structure, as will occur when there is a local temperature increase. If the increase in energy is above kT (i.e., the entire environment has not increased its temperature), the molecule will come to thermal equilibrium with the environment around it, and return to its original energy state. Which one of the following physiological process is example to this? Select one : a. Absorbance of light by 11-cis-retinal. b. Translucent to opaque conversion of egg whites after cooking. C. Absorbance of light by melanın. d. a & b e. a & c f.b&c g. a, b & carrow_forwardWhich of the following statements is true? (a) The largerthe Q, the larger the ΔG°. (b) If Q = 0, the system is at equilibrium.(c) If a reaction is spontaneous under standardconditions, it is spontaneous under all conditions. (d) Thefree-energy change for a reaction is independent of temperature.(e) If Q > 1, ΔG > ΔG°.arrow_forward
- Consider the following chemical reaction: Glucose + ATP → Glucose-6-Phosphate + ADP + Pi Given the following information, calculate the actual free energy change (G’) of this reaction. G’ of Glucose + ATP → Glucose-6-Phosphate + ADP + Pi = -16.7 kJ/mol [Glucose] = 5.0 mM [ATP] = 1.85 mM [Glucose-6-Phosphate] = 0.083 mM [ADP] = 0.14 mM [Pi] = 1.0 mM Temperature = 37 C R (Gas Constant) = 8.314 J/mol•Karrow_forwardThe primary source of phosphate for chemical reactions in cells comes as ATP, ADP, or AMP. The ΔG˚’ for the hydrolysis of ATP into ADP and Pi is -30.5 kJ/mol. Calculate the equilibrium constant for the hydrolysis of ATP.arrow_forwardThe following equation, which represents the oxidative breakdown of glucose by body cells, is a reversible reaction. Glucose + oxygen S carbon dioxide + water + ATP (a) How can you indicate that the reaction is reversible? (b) Howcan you indicate that the reaction is in chemical equilibrium? (c) Define chemical equilibrium.arrow_forward
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