Problem: Methanol (CH3OH) is used as a fuel in race cars.You may want to reference (Pages 187 - 190) Section 5.7 while completing this problem.Write a balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product.  Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. (Refer to Appendix C (Pages 1088 - 1091) to find the respective standard enthalpies of formation.)   Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g/mL.Calculate the mass of CO2 produced per kJ of heat emitted.

FREE Expert Solution

Step 1

2 CH3OH (l) + 3 O2 (g) 2 CO2 (g) + 4 H2O (g)

Reactant       Product

C          2                   2

H          8                   8

O          8                   8

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Problem Details

Methanol (CH3OH) is used as a fuel in race cars.

You may want to reference (Pages 187 - 190) Section 5.7 while completing this problem.

Write a balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product.

Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. (Refer to Appendix C (Pages 1088 - 1091) to find the respective standard enthalpies of formation.)

Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g/mL.

Calculate the mass of CO2 produced per kJ of heat emitted.

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 Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Curtis' class at UNC.