Ammonium cation NH4 dissociate in diluted aqueous solution according to the scheme: NH4+H2O →→→ NH3 + H30* At 25 °C ammonium cation has pKA = 9.245 and its standard dissociation enthalpy AH = 52.01 kJ mol-¹. زومان 26 a) Is the dissociation of ammonium cation exothermic or endothermic? b) Consider, without calculation, if ammonia (NH3) is stronger or weaker base at higher temperature

Ammonium cation NH4 dissociate in diluted aqueous solution according to the scheme: NH4+H2O →→→ NH3 + H30* At 25 °C ammonium cation has pKA = 9.245 and its standard dissociation enthalpy AH = 52.01 kJ mol-¹. زومان 26 a) Is the dissociation of ammonium cation exothermic or endothermic? b) Consider, without calculation, if ammonia (NH3) is stronger or weaker base at higher 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 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...

See similar textbooks

Similar questions

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.
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
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.
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.
C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst
For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 3O2(g) ⟷⟷ 2Fe2O3(s) ΔSo = –549.73 J∙K–1 at 298 K. The enthalpy of formation of Fe2O3(s) is –824.2 kJ∙mol–1. What is the standard change in Gibbs free energy for this reaction at 298 K? A)-660 kJ B)-1,485 kJ C)-988 kJ D)-1,812 kJ
15. When a solute is able to go spontaneously into solution: (A) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always positive. (B) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always negative. (C) the enthalpy (AHsoln) is always negative, while the entropy (Scoln) is always positive. (D) the enthalpy (AHsoln) may be positive or negative, but the entropy (ASsoln) is always positive. (E) the enthalpy (AHsoln) is always negative, but the entropy (ASsoln) may be positive or negative.
) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?,co (»= -26.41 kcal/mol, AH9,cH,0H(0)= -48.08 kcal/mol, AG,co ()= -32.8079 kcal/mol, AG?.cH,oH()= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where C§ is in cal/mol-K and T is in K |Component CH;OH CO b x10 с х105 -0.291 0.1283 a d ×10" 4.55 6.726 2.186 0.04 -0.0457 -1.92 -0.5307 -0.2079 6.952 0.09563
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C,H, (g) + H, (g) =2CH,(g) the standard change in Gibbs free energy is AG° -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pc,H6 0.250 atm, PH, = 0.150 atm, and PCHA = 0.750 atm? AG = 2.057 kJ/mol Incorrect