Dry reforming is a novel reaction concept combines two greenhouse gases (CO2 and CH4) to produce CO and H2 (termed synthesis gas since these two molecules can be used as the building blocks to produce many other petrochemical chemicals). The reaction follows: CO2 + CH4 S 2H2 + 2CO (50 – 100 atm, 250 °C) The thermochemical data for each of the species at 1000 K are: CO2 CH4 Н CO AH;° (kJ/mol) -360.11 -36.42 20.68 -88.85 s° (J/mol-K) 166.22 269.30 249.95 234.53 (1) What are the heat of reaction, entropy of reaction, and the Gibbs free energy of reaction at this temperature (i.e., 1000 K)? Please include the appropriate units. (2) What is the gas phase equilibrium constant at 1000 K? (3) If the reaction is carried out at 0.5 atm and equal molar of carbon dioxide and methane are fed, what is the equilibrium conversion under this condition (0.5 atm and 1000 K)? (4) To increase the equilibrium conversion at 1000 K, should we increase or decrease the reaction pressure? Why? Report the equilibrium conversion at a different pressure (other than 0.5 atm) to support your answer. (5) A researcher followed the above equilibrium analysis and attempted to carry out the reaction at the same temperature (i.e., 1000 K) and pressure (i.e., 0.5 atm) in a plug flow reactor (i.e., by feeding CO2 and CH4 into a hollow tube). However, this researcher quickly found that the actual conversion is much smaller than the calculated equilibrium conversion. Can you suggest a hypothesis why this is happening? What potential strategy you would recommend to help increase the reaction conversion?