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.

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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.

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

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