Calculate the equilibrium constants K and Kc, the degree of dissociation, alpha for the dissociation of hydrogen gas at 3000 K and 1 bar. The standard molar Gibbs energies of formation of H2(g) and H(g) at 3000 K and 1 bar are 0 and 46.0 kJ/mol, respectively. Assume ideal gas behavior. H2(g) 2 H(g)
Calculate the equilibrium constants K and Kc, the degree of dissociation, alpha for the dissociation...
step by step pls can you only do uestion 2 and 3 for me step by step From the information in the Data section of the textbook, calculate the equilibrium constant at 338 K for the reaction: assuming that the reaction enthalpy is independent of temperature. Answer: 0.0835 The degree of dissociation, a, for the following reaction is 0.655 at 298 K and 1.00 bar total pressure. Find K Answer: 300 Given K 9.18E-8 for the reaction: laqi and the...
Compute the partial pressures of all gases in this mixture. Show all work. 1. Equilibrium constants (40 points) The standard Gibbs en kl/mol, respectively. Consider an equilibrium established at this temperature and 1 bar: 2NO2(g) ergies of formation for N204(g) and NO2(9) at 298 K are 97.89 kJ/mol and 51.31 N204 (g)
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A, G, for various hstances at 298.15 K and one har 1057 Substance Formula 4,6°/kJ-mol- acetylene ammonia C.H,() NH,(g) CHCI) Br(e) CH) C(s) C(s) CO (8) CO(g) 209.20 - 16.367 124.35 3.126 -17.15 2.900 benzene bromine butane carbon(diamond) carbon(graphite) carbon dioxide carbon monoxide ethane ethanol ethene glucose hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen peroxide iodine methane methanol CH(E) сHOH(1) CH (8) CH...
At 248 ºC and a total pressure of 1.00 atm the degree of dissociation of SbCl5(g) is alpha = 0.718 for the reaction SbCl5(g) ↔ SbCl3(g) + Cl2(g) . The degree of dissociation alpha is defined as: alpha = (number of moles of SbCl5 dissociated at equilibrium) / (original number of moles of SbCl5) . (a) What is the value of the equilibrium constant K(T) at 248 ºC and 1.00 atm? (b) What is the value of Kx (the equilibrium...
At 248 ºC and a total pressure of 1.00 atm the degree of dissociation of SbCl5(g) is alpha = 0.718 for the reaction SbCl5(g) ↔ SbCl3(g) + Cl2(g) . The degree of dissociation alpha is defined as: alpha = (number of moles of SbCl5 dissociated at equilibrium) / (original number of moles of SbCl5) . (a) What is the value of the equilibrium constant K(T) at 248 ºC and 1.00 atm? (b) What is the value of Kx (the equilibrium...
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 = 1.83 bar PSi2H6 = 0.96 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). ΔGf(Si2H6) = 127.3 kJ/mol ΔGf(H2) = 0 kJ/mol
1--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? CH4 (g) + 2 O2 (g) ⇌ CO2 (g) + 2 H2O (g) The conditions for this reaction are: PCH4 = 0.73 bar PO2 = 0.27 bar PCO2 = 0.10 bar PH2O = 1.41 bar 2--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 =...
8. Given the following bond dissociation energies, what is the AF" for the formation of hydrogen chloride? H2(g) + Cl2(g) → 2 HCI(g) Bond Energy (kJ/mol) Bond 436 243 432 H-H Cl-CI H-Cl A) 185 kJ/mol. B) -92.5 k.J/mol. C) 92.5 kJ/mol. D) -185 kJ/mol.? E) 277.5 kJ/mol.
1. The simplest ammonia formation is from nitrogen and hydrogen. Consider the reversible reaction N2(g) + 3H2(g) → 2NH3(g) The standard enthaply and Gibbs free energy of formation one mole NH3 is ∆H◦ m = −46.11 kJ mol−1 and ∆G◦ m = −16.78 kJ mol−1 . (a) What is equilibrium constant at standard condition (25°C and 1 atm)? (b) What is equilibrium constant at 60°C and 1 atm? (c) What is the Gibbs free-energy change relative to that under standard...
What is the equilibrium constant of the formation reaction of ammonia gas at 298.15 K under the conditions that the partial pressures of N2, H2 and NH3 are 2.00 bar, 3.00 bar, and 2.00 bar, respectively? (Hint: Be careful! This is a trick question! The equilibrium constant is what it is. It is not dependent on what the partial pressures happen to be at any particular time. K is purely dependent on the standard Gibbs free energy of the reaction..)