Determine the molar Gibbs energy of mixing for the formation of a mixture of two perfect gases (A and B) at a temperature of 252 K. The mole fraction of gas A is XA = 0.466. AGm =. kJ mol-1 (± 0.2 kJ mol-1)
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- Without doing a calculation, decide whether the presence of (a) attractive, (b) repulsive interactions between gas molecules will raise or lower the molar Gibbs energy of a gas relative to its 'perfect' value.The change in the Gibbs energy of a certain constant-pressure process was found to fit the expression delta(G) /J = -73.1 + 42.8(T/K). What is the value of delta(S) for the process.A mixture of ideal gases consist of the following gases by mole fraction 10% CO2 60% H2O and 30% CO. Determine the Gibbs function of the CO in this mixture when the mixture pressure is 9.00 ATM and it's temperature is 800 Kelvin use data from the tables.
- Hydrogen gas can be produced from the reaction of graphite and steam according to the following reaction: C(s, graphite) + H2O(g) - CO(g) + H2(g) K = 2.77x10-4 at 650 K 2.67 bar of gaseous H20 and excess graphite are added to a sealed container and then heated to 650 K. What is the partial pressure of gaseous H2, in units of bar, when the system reaches dynamic equilibrium?3.12 The standard molar entropies of water ice, liquid, and vapor are 37.99, 69.91, and 188.83 J K-' mol"', respectively. On a single graph, show how the Gibbs energies of each of these phases vary with temperature.Hydrogen gas can be produced from the reaction of graphite and steam according to the following reaction: C(s, graphite) + H20(g) = CO(g) + H2(g) K= 2.77x10-4 at 650 K 6.27 bar of gaseous H20 and excess graphite are added to a sealed container and then heated to 650 K. What is the partial pressure of gaseous H2, in units of bar, when the system reaches dynamic equilibrium? Your Answer: Answer Answer units
- A sample of water vapour at 200 °C is compressed isothermally from 288 cm³ to 67 cm³. What is the change in its molar Gibbs energy? J/mol. 4 sig. figures.the repulsive Suppose that a gas obeys the van der Waals equation of state With much greater that the attractive effects. Calculate the change in molar Gibbs energy when the pressure is changed from pi to pf isothermally. Given: b = 4.566x10-5 m³/mol, R = 8.3145 J/K/mol, T = 300 K, P₁ = 1.478 bar, Pf = 3.578 bar. AGM = J/mol. 4 sig. fig.Suppose now that argon is added to the mixture in the previous exercise to bring the composition closer to real air, with mole fractions 0.780. 0.210, and 0.0096, respectively. (a) What is the additional change in molar Gibbs energy and entropy at 298 K? (b) Is the mixing spontaneous?
- In the gas phase reaction 2 A(g) + B(g) 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and A GO isFor a certain constant-pressure process, the change in Gibbs energy was found to fit the expression: G/J = -20+ 10(T/K). What are H and S for the process?At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 2 B(g) = C(g) + 2 D(g) were found to be PA 5.61 atm, PB = 4.31 atm, Pc = 5.66 atm, and P = 5.84 a %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AGixn mol