# Problem: Methanol (CH3OH) burns in oxygen to form carbon dioxide and water. Write a balanced equation for the combustion of liquid methanol and calculate ΔH, ΔS, and ΔG at 25 °C. Is the combustion of methanol spontaneous?

###### FREE Expert Solution

Balanced reaction: CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(g)

Step 1: We can use the following equation to solve for ΔH˚rxn:

Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol.

Also, note that ΔH˚f for elements in their standard state is 0.

ΔH°rxn = –637.9 kJ/mol

Step 2: We can use the following equation to solve for ΔS˚rxn:

Note that we need to multiply each S˚ by the stoichiometric coefficient since S˚ is in J/mol • K.

93% (450 ratings)
###### Problem Details

Methanol (CH3OH) burns in oxygen to form carbon dioxide and water. Write a balanced equation for the combustion of liquid methanol and calculate ΔH, ΔS, and ΔG at 25 °C. Is the combustion of methanol spontaneous?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.