d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?
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- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().Consider planet Earth as a thermodynamic system. Is Earth thermodynamically or kinetically stable? Discuss your choice, providing as many arguments as you can tosupport it.
- The reduction of iron(III) oxide (Fe,O3) to pure iron during the first step of steelmaking, 2 Fe2O3(s) 4Fe(s) + 302(g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + O2(g) → CO₂ (g) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -438. kJ/mol and -839. kJ/mol, respectively. Calculate the maximum mass of pure iron that can be produced by the combustion of 4100. kg of coke. Round your answer to 2 significant digits. kg x10 XThe reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking, 2 Fe2O3(s) 4 Fe(s) + 302 (g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + 0,(g) → CO₂ (g) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -412. kJ/mol and -836. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 470. t of pure iron. (One metric ton, symbol t, equals 1000-kg.) Round your answer to 2 significant digits. kg x10The denaturation of a biological macromolecule may be described as an equilibrium: Protein Denatured a. Show that the fraction of denatured macromolecules, 0, is related to the equilibrium constant, Kd, by K. 1+ Kd b. At pH=2, the standard enthalpy and entropy of formation for the denaturation of the enzyme chymotrypsin are 418 kJ/mol and 1.32 kJ K-' mol-', respectively. Use these data to generate a plot that shows the temperature dependence of 0. Assume the enthalpy and entropy change to be independent of temperature. c. The "melting temperature" of a biological molecule is defined as the temperature at which 0=1/2. Determine the “melting temperature" of chymotrypsin at pH=2. d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?
- The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.09 kJ mol-¹ at 2000. K and -47.35 kJ. mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AGf = 5.09 kJ mol-¹. What is K at that temperature? K at 2000. K = 5.73 K at 3000. K = Incorrect At 3000. K, AGf = -47.35 kJ · mol-¹. What is K at that temperature? IncorrectCalculate the equilibrium constant for the phosphorylation of glucose to glucose 6-phosphate at 37.0 °C. 4.74 x10¬3 M-1 eq In the rat hepatocyte, the physiological concentrations of glucose and P; are maintained at approximately 4.8 mM. What is the equilibrium concentration of glucose 6-phosphate (G6P) obtained by the direct phosphorylation of glucose by P;? 8.75 x10-8 [G6P] = M IncorrectIn the reaction 2A (g) + B(g)==>2C(g) + D(g), 3.00 mol A was mixed with 2 mol of B and 0.5 mol of D. The system was allowed to come to equilibrium. At equilibrium, 1.2 mol of C was present at a total pressure of 1 bar. Calculate the mole fractions of each species at equilibrium, K, and ΔGr at 298 K.
- Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe+302-2Fe2O3 TXn in which at 298 K, AH ASixn - 543.7 J/K. H = - 1684 kJ and Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) AGrxn Submit μÅ Value t Ć Units ?Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T' is temperature, and S is entropy. The chemical reaction that causes aluminum to corrode in air is given by 4A1+30₂-2Al₂O₁ in which at 298 K, AH = -3352 kJ and AS = -625.1J/K Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K Express your answer as an integer and include the appropriate units. ▸ View Available Hint(s) μA AG - 89 kJ Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining Part B What is the Gibbs free energy for this reaction at 5975 K? Assume that AH and AS do not change with temperature. Express your answer to two decimal places and include the appropriate units. > View Available Hint(s) ? AG= Value Units SubmitCalculate the Gibbs free energy change (AG) for the following chemical reaction: glutamate + NH3 glutamine +H2O The reaction occurs at 68 °F, the change in heat (AH) = 4103 Cal, and the change in entropy (AS)= 2.4 Cal/K. %3D