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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).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?(a) Derive an expression for the ratio of solubilities of AgCI at two different temperatures; assume that the standard enthalpy of solution of AgCI is independent of temperature in the range of interest. (b) Do you expect the solubility of AgCI to increase or decrease as the temperature is raised?
- The standard Gibbs energy of reaction at 721 K for the reaction H2(g) + I2(g) -> 2 HI(g) is ─23.6 kJ. What is the Gibbs energy at 721 K of the following reaction mixtures a) wherein the partial pressure of H2(g), I2(g) and HI(g) are 2.1 bar, 1.7 bar and 1.2- bar, respectively? b) wherein the partial pressure of H2(g), I2(g) and HI(g) are 0.62 bar, 0.23 bar and 3.2 bar, respectively? c) Interpret the results obtained for the two cases. Answer: [─29.0; +2.05]The standard Gibbs energy of formation of NH3(g) at 298 K is ─16.6 kJ mol-1. Based on this data, calculate (a) the standard Gibbs energy of reaction and (b) the pressure equilibrium concentration for the reaction N2(g) + 3 H2(g) = 2 NH3(g) Answer:[-33.2; 6.6 x 105 ]4. The standard Gibbs energy of formation of PH3(g) is l3.4 kJ/mol at 298 K. Note that the standard state of phosphorus at 298 K is P4(s). If H2(g) and PH3(g) are treated as perfect gases, and their partial pressures are both 2.0 bar: (a) What is the reaction quotient, Q? (b) What is the corresponding reaction Gibbs energy for the reaction corresponding to the standard Gibbs energy of formation of PH3(g)? (c) What is the spontaneous direction of the reaction?
- The decomposition of a generic diatomic element in its standard state is represented by the equation x,() - X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.55 kJ - mol- at 2000. K and -48.71 kJ mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG = 5.55 kJ mol-, What is K at that temperature? K at 2000. K = At 3000. K, AG, = -48.71 kJ mol-I, What is K at that temperature? K at 3000. K =The decomposition of a generic diatomic element in its standard state is represented by the equation X,(g) X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.23 kJ · mol-1 at 2000. K and –56.22 kJ · mol-1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG; = 4.23 kJ · mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG{ -56.22 kJ · mol-1. What is K at that temperature? K at 3000. K =The decomposition of a generic diatomic element in its standard state is represented by the equation x,(2) » X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.51 kJ · mol- at 2000. K and -57.84 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG; = 5.51 kJ · mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG: = -57.84 kJ . mol-1. What is K at that temperature? K at 3000. K =
- 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 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.The mean activity coefficient of a 0.2 b Mg (NO3)2 solution is 0.13 at 25oC. Calculate the mean molality, the mean ionic activity and the activity of the compound.
