Nitromethane, CH3NO2 , can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainlyCH3NO2(l) + O2(g) → CO2(g) + N2(g) + H2O(g)a. The standard enthalpy change of reaction (ΔH°van ) for the balanced reaction (with lowest whole-number coefficients) is −1288.5 kJ. Calculate ΔHf0 for nitromethane.b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

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