Ethylene gas and steam at 420 °C and atmospheric pressure are fed to a reaction process as an equimolar mixture. The process produces ethanol by the reaction: C2H4(g) + H20(g) → C2H50H(1) The liquid ethanol exits the process at 150 °C. What is the heat transfer associated with this overall process per mole of ethanol produced?
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- a sample of 98g of pure sulfuric acid is dissolved in 2.0 kg of water in an insulated vessel at 15°C, and thetemperature rises rapidly because of the process of forming the solution. The reaction is summarized in theequation H2SO4(l) -> H+(aq) + HSO4 –(aq). Estimate the temperature change assuming that the heat capacityof the solution is 4.0 J/gK and the heat capacity of the vessel is 300 J/K.The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.
- Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively Calculate the work done when 1.0 mole of nitroglycerin decomposes and additionally explain the significance of the sign.Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1.The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively. Determine the standard enthalpy of formation of 1.0 mole of nitroglycerin.To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.4500 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K.
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