CH3OH (l) + 1.5O2 (g) > CO2 (g) + 2H2O (g)
Calculate the standard enthalpy change for the reaction, assuming H2O (g) as a product.
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.
1 Answer
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Calculate the standard enthalpy change for the reaction, assuming H2O (g) as a product.
***Just use the standard heat of reactions for each substance in the balanced equation (found in appendix C if you’re using Chemistry The Natural Science), and use Hess’s Law (deltaH=sum of (number of moles)(deltaH of products) – sum of (number of moles)(deltaH of reactants).
[-393.5 + 2(-241.82)] – [-238.6 + (3/2)(0)]
= -638.54 (four sig figs = -638.5)
Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g/mL.
***Follow the units to find your answer… you want to go from g/mL to kJ/L
.791 g/mL (10^3mL/1L)(1mol methanol/32.04g)(-638.5kJ/1mol methanol)=1.58×10^4
Calculate the mass of CO2 produced per kJ of heat emitted.
***Again just use what you have and follow your units. 1 mol of CO2 is used for every 1 mol of methanol. The molar mass of CO2 is 40.010g. You divide that by the enthalpy of reaction (in kJ). This way you will end up with g/kJ.
40.010g/638.5kJ(negative sign isn’t used here) = 6.892×10^-2
Source(s): chem student, use mastering chemistry
