3. An exothermic reaction of stilbene A to form a higher-valued product trospophene B and methane C. i.e. A→B+C, was carried out adiabatically and the following data was collected: Conversion 20% 40% 45% 50% 60% 80% 90% (X) -TA 1 1.67 5 5 5 5 1.25 0.91 (mol/L/min) The entering molar flow rate of A (FAO) is 300 mol/min (a) What are the volumes of CSTR and PFR needed to achieve 20%, 40%, 60% and 80% conversion? (b) Over what range of conversion would the CSTR and PFR volumes be identical? (c) What is the maximum conversion that can be achieved in a 105-L CSTR? (d) What conversion can be achieved if a 72-L PFR is followed in series by a 24-L CSTR? (e) What conversion can be achieved if a 24-L CSTR is followed in series by a 72-L PFR?

Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process.     Question: What is the change in the system's energy during this reaction? How would your answer differ if the H2O ended up as liquid water instead of vapor?

Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process.     Question: How much heat is given off during this reaction, assuming that no "other" forms of work are done?

Consider the combustion of one mole of methane gas:CH4(gas) + 2O2(gas) --> CO2 (gas) + 2H2O(gas).The system is at standard temperature (298 K) and pressure (105 Pa) both before and after the reaction. 1.) First imagine the process of converting a mole of methane into its elemental consituents (graphite and hydrogen gas). Use the data at the back of this book to find ΔH for this process. 2.) Now imagine forming a mole of CO2 and two moles of water vapor from their elemental constituents. Determine ΔH for this process.     Question: What is ΔH for the actual reaction in which methane and oxygen form carbon dioxide and water vapor directly? Explain.

Q2/ The Gibb's free energy for the reaction CH6=CH+ H2 equals (-41.2kJ/mol) at 1200°C. Calculate the fractional conversion at 1200°C and 1.5atm if the feed contains 80% CH6, 15% H2 and 5% inert.

2 When 50 cm' of hydrochloric acid of concentration 2.0 mol dm is added to 50 cm' of sodium hydroxide solution of concentration 2.0mol dm, the temperature increase is 13.0°C HCl(aq) + NAOH(aq) + NaCl(aq) + H,O(1) The experiment is repeated using 25 cm of the same hydrochloric acid and 50 cm' of the same sodium hydroxide solution. What is the temperature increase? O A 4.9°C I B 6.5°C I C 8.7°C D 13.0°C

Please don't provide handwritten solution ...

A process for ethanol synthesis has been developed and the ethylene hydration operating conditions have been optimized in order to reduce production costs (Ayaou et al., 2019). Ethanol is manufactured by reacting ethylene with steam at 150 °C (423.15 K). The reaction takes place in a gas phase and the formation of the ethanol is an exothermic process and assume as ideal gases. ?2?4 (?) + ?2?(?) → ?2?5??(?) Your classmate claims that the equilibrium constant decreases as the temperature decreases. Evaluate the effect of reducing the temperature to 100 °C whether this observation make sense. Support your answer with the necessary calculations. Available information for the calculation are as follows ∆?? ∆?? ∆?? ∆?? ΔHo298 (J/mol) ΔGo298 (J/mol) -1.376 4.157X10-3 -1.610X10-6 -1.210X10+4 -45,792 -8,378

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6) Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm³ at 298.15 K to 2.00 dm³.