Nitric oxide (NO, MW = 30.1) reacts completely with gas phase water to form ammonia (NH3) and oxygen gas. The reactants are fed in a stoichiometric ratio at 155 °C and leave at 232.00 °C. The feed rate of NO is 2.35 g/s. Species NO AH (25 °C) kJ/mol Ср 90.4 3.5R H₂O(g) -241.8 5R NH2(g) -46.2 4.5R 02 0 3.5R Calculate the heat interaction term. 190.78 Q = Incorrect kW

29.2 Hydrogen sulfide (H₂S) is a common contaminant in natural gas. The dissolution of H₂S gas in water is a linear function of partial pressure, as is described by Henry's law of the form PA = H x. Values of H vs. temperature are provided below: T (°C) H (atm) mole H₂S/ mole MEA 20 483 PA (mm Hg) 30 449 Given the relatively low solubility of H₂S in water, an amine- based chelating agent is added to the water to improve the solubility of H₂S. Equilibrium distribution data for H₂S in a 15.9 wt% solution of monoethanolamine (MEA) in water at 40°C is provided below: 40 520 50 577 0.000 0.125 0.208 0.362 0.643 0.729 0.814 0.00 0.96 3.00 9.10 43.1 59.7 106 Describe the effect of temperature on the solubility of H₂S gas in water. b. Prepare equilibrium distribution plots, in mole-fraction coordinates (y₁ -— XÃ), for the solubility of H₂S in water vs. H₂S in 15.9 wt% MEA solution at 40°C and 1.0 atm total system pressure. Comment on the relative solubility of H₂S in water vs. MEA solution.

(d) Determine the weight percentage, wt%, of the solid solution and liquid solution of a Cu-Ni alloy with a composition of 21 % Ni 79 % Cu, at a temperature of 1050 °C. Use part of the Thermal Equilibrium Diagram for Copper (Cu)-Nickel (Ni) alloy, as shown in Figure 1. Clearly show all your calculations. Temperature "C Figure 1 Part of the Cu-Ni thermal equilibrium diagram (not to scale) 1050 11 21 29 % Ni

P2

The fuel in the form of biogas (65%-mol CH4 and 35%-mol CO2) is burned in a furnace. In order for combustion to take place stoichiometrically, calculate the air to fuel ratio (vol/vol) from this problem!

Use the information about three gases, with the properties below to answer the following questions. Nitrogen (N2) Oxygen (02) Argon (Ar) 93.0 °C 83.0 °C 73.0 °C M (kg/kmol) 28 32 40 Use the van der Waals equation of state and mixing rules to calculate the temperature where 100 kmol of a mixture of argon (10 mol%), nitrogen (45 mol%) and oxygen (45 mol %) would occupy 46.27 m³, at a pressure of 6.28 MPa. It is known that the van der Waals constant for nitrogen are a=1.370 atm(m³/kmol)² and b=0.0387 m³/kmol, and for oxygen are a=1.382 atm(m³/kmol)² and b=0.03186 m³/kmol. 63.0 °C Tc (K) 126.2 154.6 150.8 Pc (atm) 33.5 49.8 48 @ 0.04 0.021 -0.004

A thermophilic organism can also obtain energy through alcoholic fermentation according to the equation (same as above): C6H12O6(s) -→ 2C2H5OH() + 2CO2(g) Using the information below, calculate the most exact molar Gibbs energy (A,G") for the reaction at 95.0°C. (to save time, it is OK to transfer some values calculated from problem 8) Compound C.H1:O6 (s) CH$OH () CO2 (g) A,G° (kJ/mol) A,H° (kJ/mol) -1,273.3 S° (J/mol-K) Cp (J/mol-K) -910.6 210.3 219.2 -174.2 -277.0 161.0 112.3 -394.4 -393.5 213.6 37.10