Ethanol is dehydrogenated to produce acetaldehyde: C2H5OH(v) → CH3CHO(v) + H2 (g) in a continuous adiabatic reactor. Ethanol vapor is introduced into the reactor reaction at 400oC, shows that the conversion of ethanol is 30%. Find the temperature of the product using the formula of heat capacity,

The heat capacities for each of the substances involved for a particular reaction are given below. The enthalpy change for the same reaction at 298 Kelvin is -282.987 KJ/mole. From these, answer the questions that follow. Temperature-Dependence of the heat capacities of the Substances for the given reaction + (1/2)02(9) → CO2(9) For the gaseous reaction; CO the heat capacities are: Cp°co P(g) 26.86 + 6.97 x10-3 T - 8.20 x10-7 T2 %3D Cp°o2 25.72 + 12.98 x10-3 T - 38.60 x10-7 T² %3D Cp°co2 26.00 + 43.50 x10-3 T 148.32 x10-7 T² %3D What would be the overall enthalpy change at 1,000 Kelvin (AH @ 1000K, in KJ)?

Isopropanol, with 13 wt% water, can be dehydrated to obtain almost pure isopropanol at a 90% recovery by azeotropic distillation with benzene. When condensed, the overhead vapor from the col- umn forms two immiscible liquid phases. Use Table 2.4 with data in Perry's Handbook and the data below to compute the heat-transfer rate in Btu/h and kJ/h for the condenser. Water-Rich Organic-Rich Overhead Phase Phase Phase Vapor Liquid Liquid Temperature, °C 76 40 40 Pressure, bar 1.4 1.4 1.4 Flow rate, kg/h: Isopropanol 6,800 5,870 930 Water 2,350 1,790 560 Benzene 24,600 30 24,570

. CO₂ entering from a combustion (T = 500°C) process is mixed stoichiometrically with H₂ at (T= 25°C). A reaction occurs over a catalyst producing water and methane with a 70% conversion of the reactants. If the products leaving the reactor have a temperature of 725°C calculate the heat transfer to or from the reactor. CO₂ + 4H₂ → 2H₂O+CHA Assume Constant Cp for all components except H₂O. kJ mole. C CO2: Cp= 0.037 kJ mole C CO₂ T = 500°C H₂ T = 25°C H2: Cp = 0.029. Reactor kJ mole. C CH4: Cp = 0.033- CO2, H2, H₂O, CH4 T = 725°C