The dissociation vapor pressure of a salt A2B(s) A2ig) + B(g) at 367°C is 208 kPa but at 477°C it has risen to 547 kPa. For the dissociation reaction of A2B(5), calculate (i) the equilibrium constant, (ii) the standard reaction Gibbs energy, (iii) the standard enthalpy, and (iv) the standard entropy of dissociation, all at 422°C. Assume that the vapor behaves as a perfect gas and that A,H° and A,S° are independent of temperature in the range given.

The dissociation vapor pressure of a salt A2B(s) A2ig) + B(g) at 367°C is 208 kPa but at 477°C it has risen to 547 kPa. For the dissociation reaction of A2B(5), calculate (i) the equilibrium constant, (ii) the standard reaction Gibbs energy, (iii) the standard enthalpy, and (iv) the standard entropy of dissociation, all at 422°C. Assume that the vapor behaves as a perfect gas and that A,H° and A,S° are independent of temperature in the range given.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(b) CMC of a surfactant in water at 25 °C is 0.5 g L-¹ and at 45 °C is 0.3 g L-1. The molar mass of the surfactant is 110 g mol-¹. (i) Calculate: The Gibbs energy of micellisation, AGO, of the surfactant at 25 °C and 45 °C, The fractions (%) of the surfactant molecules in free and in micellar states in 0.5 g L-¹ aqueous solution of the surfactant and temperature 45 °C. ● ● (ii) Calculate CMC for the surfactant in water at 55 °C.
Basing on the standard Gibbs energy of formation, determine if the hydrogenation of benzene to cyclohexane, i.e. C6H6(1) + 3 H2(g) →→ C6H12(1) is feasible. [-97.8] 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
The reaction of ozone in the atmosphere and nitric oxide has a reaction enthalpy and reaction entropy of -199 kJ mol-1 and -4.1 J K-1 mol-1, respectively. What is its reaction Gibbs energy at 25 °C? O3(g) + NO(g) → NO2(g) + O2(g) 1220 kJ mol-1 -200 kJ mol-1 -1420 kJ mol-1 -198 kJ mol-1
11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid. (b) Determine the pH of 0.100 mol dm–3 NaOH at 298 K [pKw = 14.0].
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 =
An aqueous solution of 43.80 mL of 0.240 mol L-1 NaCN is added to 43.80 mL of 0.240 mol L-1 Zn(NO3)2(aq) at 25oC. Determine the concentration (in mol L-1) of Zn(CN)42- in the solution once it reaches thermodynamic equilibrium at 25oC. Kf(Zn(CN)42-)=2.1×1019
Consider the dissolution of calcium fluoride: CaF2(s) → Ca?*(aq) + 2 F(aq) Part B which has the following standard enthalpy and entropy of reaction: At 368.3 K, the solubility of calcium fluoride is 3.32×10¬4 mol L-1. Compute the Gibbs energy change (A,G) for the reaction if this saturated solution is suddenly cooled to 275.0 K. 1 A:H° = 14.4 kJ mol- A,S° = -149.2 J K-1 mol-1 17.6 kJ mol-1 -10.7 kJ mol-1 0.0 kJ mol-1 25.2 kJ mol-1 3.6 kJ mol-1
Calculate the standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s) and the standard Gibbs energy and enthalpy of the cell reaction at 25 °C. (ii) Estimate the value of A,GE at 35 °C.
Calculate the standard Gibbs energy change for the following reaction at 298 K H2(g) + Cl2(g) ® 2HCl(g) [DfHo = –92.3 kJ mol–1 for HCl; S in J K–1 mol–1 is 131, 223, and 187 for H2, Cl2 and HCl, respectively].
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 =
Physical Chem #4