Methanol is synthesized commercially from CO and H2 by the reaction, CO + 2H2 ----> CH3OH over a Cu/ZnO catalyst at 350 C at 50-100 atm. The standard-state thermodynamic data on this reaction are deltaHR,298 = -90.64 kJ/mole and deltaGR,298 = -24.2 kJ/mole. a) What is the equilibrium conversion of a stoichiometric mixture of CO and H2 to methanol at 298 K at 1 atm? b) Assuming deltaHR independent of T, what are Keq and the equilibrium conversion at 1 atm and 350 C? c) The actual value of Keq at 350 C is 1.94*10^-4. How large is the error assuming constant deltaHR? d) At what pressure will the equilibrium conversion be 50% at 350 C?