Partial oxidation of methane with excess of oxygen takes place at 1 atm and 200°C in a continuous tubular reactor, according to R1: C H_{4}(g)+\frac{3}{2} O_{2}(g) \rightarrow C O(g)+2 H_{2}

O(g) The reactor is designed to reach a 50% fractional conversion of a vChala)in= 200 L min-1 methane inlet, xCHa(g)= 0.5. Assuming ideal gas behaviour, (i) Calculate the mass of water produced after one day and molar flow of carbon monoxide produced per second, in absence of any other lateral reactions.[8 marks] In order to fulfil H&S regulations, a more oxidizing atmosphere is generated, to promote further oxidation of CO(g) to CO2(g), according to R2: C O(g)+\frac{1}{2} O_{2}(g) \rightarrow C O_{2}(g) Under these conditions of temperature and pressure, a sensor is installed at the outlet stream, which is set to stop the process at a maximum value of vco(g).out= 1000 L s-1. For this limiting threshold, and at the same inlet and fractional conversion of methane as in the previous section of the question (as well as stoichiometry), Calculate the minimum amount of air needed in m3 · h-1. ii) Selectivity of CO2(g) produced respect to CO (g). (iv) Estimate the heat released or absorbed in the reactor, neglecting the specific enthalpies at the inlet and outlet streams.[5 marks]