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11 Nov 2019

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.

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Bunny Greenfelder
Bunny GreenfelderLv2
24 May 2019

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Related questions

Ammonia (NH3) boils at –33 °C; at this temperature it has a density of 0.81 g/cm3. The enthalpy of formation of NH3(g) is –46.2 kJ/mol, and the enthalpy of vaporization of NH3(l) is 23.2 kJ/mol. Calculate the enthalpy change when 1 L of liquid NH3 is burned in air to give N2(g) and H2O(g). How does this compare with ∆H for the complete combustion of 1 L of liquid methanol, CH3OH(l)? For CH3OH(l), the density at 25 °C is 0.792 g/cm3, and ∆Hf° = –239 kJ/mol.

Methanol is manufactured by the partial combustion of methane under pressure, using a copper catalyst:
CH4(g) + ½ O2(g) → CH3OH(l)
Enthalpies of combustion are (in kJ mol-1):

CH4(g), -881
CH3OH(l), -726

Calculate the standard enthalpy change for the manufacture of 1 mole methanol by the reaction
CH4(g) + ½ O2(g) → CH3OH(l)

Follow the procedures based on Hess’s Law:
First write down the reactions corresponding to the enthalpies of combustion you have been given, reverse one of the equations remembering to change the sign of ΔHo, then combine these equations to give the required process, and evaluate the associated ΔHo
State the answer to three significant figures without decimal point, ±xxx

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