The enthalpies of formation of CO(g) and CH3OH(l), respectively, are -110.5 and -239.1 kJ
mol–1. Calculate the enthalpy of the reaction above that forms methanol from synthesis gas.
From your answer, predict whether the equilibrium amount of methanol obtained will
increase or decrease as the temperature is lowered. Given your result, comment on the
interest in developing low-temperature catalysts.    

The enthalpies of formation of CO(gas) and CH3OH (liquid) are -110.5 and -239.1 kJ/mol, respectively. Calculate the enthalpy of the syngas reaction to form methanol. Predict weather the equilibrium amount of methanol will decrease or increase with increasing temperature of the process.

The equation for the combustion of gaseous methanol is

(a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol?

(b) Compare your answer in part (a) with the value of Δ_rH° calculated using enthalpies of formation data.