A vapour-liquid mixture of water (1) and furfural CSHAO2 (2) is °C. Under these conditions, it is found that x1 = 0.10 and y1 = 0.81. The temperature of the mixture is changed to 100.6 °C, and some (but not all) of the vapour condenses. The vapour phase may be assumed to behave as an ideal gas. The liquid-phase activity coefficients are independent of temperature but vary with concentration according to the van Laar equations. Determine: (a) The activity coefficients for water and furfural at 1.013 bar and 109.5 °C [9% ) (b) The van Laar constants [6%] Vapour pressure data: T=100 6°C. Pal -1.0352 bar, Pal -0.1193 bar

Use the R-K equation of state to estimate the partial fugac- ity coefficients of propane and benzene in the vapor mixture of Example 2.5.

Derive an expression for the molar excess enthalpy of mixing of a mixture described by a molar excess Gibbs free energy of the form gE = X1X2(A21X1 + A12X2) where the constants A21 and A12 are independent of temperature.

X Your answer is incorrect. Liquid ethanol (CH;OH) at 25°C, 1 atm enters an insulated reactor operating at steady state and burns completely with air entering at 370 K, 1 atm. The combustion products exit at 1300 K. Kinetic and potential energy effects can be neglected and the air can be modeled as 21% O, and 79% N2 on a molar basis. Determine the percent excess air used. 51

Ethylene gas is converted ethanol compound by vapor phase hydration reaction. is being transformed. Maximum conversion amount at 523 K and 35 bar conditions, Calculate based on the amount of steam being 5 times the amount of ethylene. gas in equilibrium Assume that the mixture exhibits ideal solution behavior.

Consider the following chemical equilibrium: HCOOH(aq) + H_2O(aq) \rightleftharpoons HCOO^-(aq) + H_3O^+(aq). Which of the following graphs represents the perturbation on the system and the change of pH when water is evaporated from the container?

Calculate the Gibbs free energy of fusion (melting) for water [in J/mol] at T = 0°C at 15.0 bar noting that it is zero at 1.0 bar. Assume the densities of the two phases are 1.000 g/cc (liquid) and 0.9150 g/cc (solid).

Suppose that a hydrogen fuel cell, as described in the text, is to be operated at 75° C and atmospheric pressure. We wish to estimate the maximum electrical work done by the cell, only the room-temperature data at the back of this book. It is convenient to first establish a zero-point for each of the three substances,H2 , O2, and H2O. Let us take G for both H2 and O2 to be zero at 25°C, so that G for a mole of H20 is -237 kJ at 25°C.(a) Using these conventions, estimate the Gibbs free energy of a mole of H2 at 75°C. Repeat for O2 and H2O.(b) Using the results of part (a), calculate the maximum electrical work done by the cell at 75°C, for one mole of hydrogen fuel. Compare to the ideal performance of the cell at 25°C.

A popular commercial solvent mixture is made up of several aliphatic and aromatic hydrocarbons.You are tasked with estimating its properties assuming toluene is the main component.You are expected to solve this problem in two ways, a) using the Lee-Kesler diagrams to estimate the following quantities. A) The molar volume at the critical point.B) The molar volume in the liquid phase at T = 110C and P = 10 bar.C) The molar volume in the vapor phase at T = 310C and P = 20 bar.D) The change in molar enthalpy when toluene is heated and compressed from T = 110C andP = 10 bar to T = 310 C and P = 20 bar.Note: you may use PREOS and other Excel spreadsheets, but only as a calculator

Please answer sub-part d. Thank you so much.