3) Thermophiles are single-cell organisms that live by deep sea hydrothermal vents. The temperatures of the vicinity of the vent can reach 122 °C. The dissociation of water has a standard enthalpy of 55.82 kJ mol-1. What is the pH of water at 122 °C? (You may assume the AHO is independent of temperature).

3) Thermophiles are single-cell organisms that live by deep sea hydrothermal vents. The temperatures of the vicinity of the vent can reach 122 °C. The dissociation of water has a standard enthalpy of 55.82 kJ mol-1. What is the pH of water at 122 °C? (You may assume the AHO is independent of temperature).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 83QRT: Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate,...

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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.
For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), the standard enthalpy of reaction ARH° is -197.8 kJ, and the standard entropy of reaction ARS is -188.0 J K¹. At what temperature will this reaction be at equilibrium? [1052] Standard Gibbs energy of formation, in kJ mol-¹, at 25°C Benzene, C6H6(1) + 124.5 Carbon dioxide, CO2(g) - 394.4 Carbon monoxide, CO(g) - 137.2 Cyclohexane, C6H₁2(1) + 26.7 Ethanoic acid, CH3COOH (1) - 299.8 Ethanol, C₂H5OH(1) - 174.8 Water, H₂O(1) -237.1
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
Some H2CO3 and HCO3- are added to water such that the concentration of each is the same value, 12.0 mmol L-1 (pKa = 6.3, 10.3). The water was initially at pH 7.05 and 25.0 °C. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)
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Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
The Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).
Σ II For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N,(g) + 3 H, (g) = 2 NH, (g) the standard change in Gibbs free energy is AG° = –32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.450 atm, PH, = 0.250 atm, and PNH = 0.650 atm? kJ/mol = 9V 50:8 11/8 PrtScr Insert Delete F10 F11 F12 F7 F4 KA & Backspac 24 % 60 H. B.
Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?
The standard Gibbs energy of formation of gaseous ozone at 25.0 ℃ ΔfGo, is162.3 kJ. mol-1, for standard state of 1 bar. The reaction is: 3O2 (g) ⇌ 2O3(g). Calculate the value of Kx at 2 bar.
The standard enthalpy of combustion of the solid glycine (the amino acid, NH2CH2COOH) is −969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1. Calculate the standard Gibbs energy of formation of glycine at 298 K. Note that the nitrogen-containing species produced on combustion is taken to be N2(g).
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