The ∆G° of vaporization for cyclohexane at 298 K and 1.00 atm is -0.2164 kJ/mol. Calculate the pressure, in atm, of cyclohexane vapor in equilibrium with cyclohexane liquid at 298 K.
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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.free energy and equilibriumA spontaneous reaction always has: A. a positive enthalpy change and a negative entropy change. B. a positive Gibbs free energy change. C. a negative Gibbs free energy change. D. a standard enthalpy of formation equal to zero for one of the reactants. E. a standard free energy of formation equal to zero for one of the reactants.
- 3. A reaction has a standard free energy change (G⁰) of -21.6 kJ/mol at 25 ⁰C.a. Is this reaction spontaneous or non-spontaneous at 25 ⁰C? b. Given the value of G⁰ above (-21.6 kJ/mol), what is the value of the equilibrium constant (K or Keq)for this reaction at 25 ⁰C?If the ▲G0 for a reaction is -4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the change in entropy of this reaction if ▲H0 = -3.2 kcal/mol?TRUE OR FALSE The spontaneous process proceeds on its own without any outside assistance.
- What is the entropy at SATP of a reaction where ∆Hºrxn=-12.5 kJ and Keq=32.1? -0.150 J/K -150 J/K -29.4 J/K -13.1 J/KCalculate ΔS° for the reaction of H2(g) with liquid benzene (C6H6) to give cyclohexane (C6H12). ?° H2 = 130.68 J/mol K ?° C6H6 = 173.4 J/mol ∙ K?° C6H12 = 204.4 J/mol∙ K Answer should be -361.1 J/KIf a reaction occurs rapidly it is spontaneous. True or false
- Determine whether each of the following statements about the thermodynamic functions are True or False as they apply to chemical reactions. True False Negative enthalpy changes increase spontaneity. True False The heat of reaction at constant volume is never equal to the heat of reaction at constant pressure. True False Entropy and enthalpy are included in the Gibbs free energy. True False All spontaneous chemical reactions have negative heats of reaction. True False Spontaneity is increased by positive entropy changes.How do I answer these questions? 1. For a reaction that has ∆H of -30 kJ and ∆S of -62 J/K, estimate at what temperature will the reaction change from spontaneous to non-spontaneous reaction? 2. For a reaction glutamate + NH3 → glutamine + H2O that occurred at 20⁰C, calculate the Gibbs free energy change of the reaction. Given the change in enthalpy of 3103 cal and change of entropy of 3.4 cal/K. 3. For a reaction of conversion of ATP into ADP at 20⁰C, calculate the reaction Gibbs free energy. Given the change in enthalpy is 20.27 Kcal and the change in entropy is 85 cal/Kelvin.The ∆G° of vaporization for propane at 298 K and 1.00 atm is -6.602 kJ/mol. Calculate the pressure, in atm, of propane vapor in equilibrium with propane liquid at 298 K.